This document provides an outline for a chemistry lecture covering several topics:
1) Chemistry is the study of matter, its composition, properties, and transformations. Matter can exist in solid, liquid, or gas states.
2) The three states of matter - solid, liquid, gas - are defined by their characteristic properties regarding shape and particle movement.
3) All matter can be classified as either a pure substance or a mixture. Pure substances are either elements or compounds.
This document provides an overview of key concepts in chemistry. It discusses how chemistry connects the macroscopic world we experience to the microscopic world of atoms and molecules. Matter is composed of tiny particles called atoms, which combine to form molecules. A chemical reaction involves rearranging the way atoms are attached to each other. The three common states of matter are solids, liquids, and gases. Physical changes alter the form of matter without changing its chemical makeup, while chemical changes create new substances.
1. Chemistry is the study of matter and its properties and changes. It impacts many areas including health, energy, materials, food and agriculture.
2. Matter can be classified as elements, compounds or mixtures. Elements cannot be broken down further, compounds are made of two or more elements chemically bonded together, and mixtures maintain their individual identities.
3. The three main states of matter are solids, liquids, and gases. Physical and chemical changes alter or do not alter the composition of matter. The scientific method is used to study chemistry through observation, hypothesis, experimentation and theory development.
This document provides objectives and information about scientific measurement. It discusses accuracy, precision and error in measurements. It defines significant figures and how to determine them. It explains how to properly handle significant figures in calculations and addresses rounding. The document also discusses the International System of Units (SI) including base units like meters, kilograms and kelvin. It covers density, how it is calculated from mass and volume, and how density varies with temperature for most substances.
1) Chemistry is the study of matter and its properties. Matter can exist as solids, liquids, or gases and can undergo physical or chemical changes.
2) The metric system is the international standard for measurement and uses base units related by powers of 10. Measurements include mass, volume, length, and temperature.
3) Energy exists in various forms and can be transformed from one to another but not created or destroyed. Chemical energy is stored in chemical bonds and released during chemical reactions.
1) The document discusses units of measurement and the International System of Units (SI). It describes the seven base SI units including meters, kilograms, and seconds.
2) Derived units are combinations of base units, such as cubic meters for volume. Density is defined as the ratio of mass to volume.
3) Conversion factors allow quantities to be converted between units, using dimensional analysis. Sample problems demonstrate converting between grams, milligrams, and kilograms.
the mathematics of chemistry stoichiometry dimensional analysis.pptjami1779
Here is a stoichiometry question I wrote for the given reaction:
If 3.25 grams of barium chloride are available to react, how many grams of barium sulfate can be produced?
Chemistry is the study of matter, its properties, and the changes it undergoes. Matter is anything that has mass and takes up space, and is composed of atoms. Atoms are the building blocks of matter and each element is made of the same type of atom. Compounds are made of two or more different elements chemically bonded together. Mixtures contain two or more substances mixed but not chemically combined. Measurements in chemistry use significant figures and units to accurately quantify properties and changes in matter.
Chemistry is the study of matter, its properties, and the changes it undergoes. Matter is anything that has mass and takes up space, and is composed of atoms. Atoms are the building blocks of matter and each element is made of the same type of atom. Compounds are made of two or more different elements chemically bonded together. Mixtures contain two or more substances mixed but not chemically combined. Measurements in chemistry use significant figures and the SI system of units including meters, grams, and liters.
This document provides an overview of key concepts in chemistry. It discusses how chemistry connects the macroscopic world we experience to the microscopic world of atoms and molecules. Matter is composed of tiny particles called atoms, which combine to form molecules. A chemical reaction involves rearranging the way atoms are attached to each other. The three common states of matter are solids, liquids, and gases. Physical changes alter the form of matter without changing its chemical makeup, while chemical changes create new substances.
1. Chemistry is the study of matter and its properties and changes. It impacts many areas including health, energy, materials, food and agriculture.
2. Matter can be classified as elements, compounds or mixtures. Elements cannot be broken down further, compounds are made of two or more elements chemically bonded together, and mixtures maintain their individual identities.
3. The three main states of matter are solids, liquids, and gases. Physical and chemical changes alter or do not alter the composition of matter. The scientific method is used to study chemistry through observation, hypothesis, experimentation and theory development.
This document provides objectives and information about scientific measurement. It discusses accuracy, precision and error in measurements. It defines significant figures and how to determine them. It explains how to properly handle significant figures in calculations and addresses rounding. The document also discusses the International System of Units (SI) including base units like meters, kilograms and kelvin. It covers density, how it is calculated from mass and volume, and how density varies with temperature for most substances.
1) Chemistry is the study of matter and its properties. Matter can exist as solids, liquids, or gases and can undergo physical or chemical changes.
2) The metric system is the international standard for measurement and uses base units related by powers of 10. Measurements include mass, volume, length, and temperature.
3) Energy exists in various forms and can be transformed from one to another but not created or destroyed. Chemical energy is stored in chemical bonds and released during chemical reactions.
1) The document discusses units of measurement and the International System of Units (SI). It describes the seven base SI units including meters, kilograms, and seconds.
2) Derived units are combinations of base units, such as cubic meters for volume. Density is defined as the ratio of mass to volume.
3) Conversion factors allow quantities to be converted between units, using dimensional analysis. Sample problems demonstrate converting between grams, milligrams, and kilograms.
the mathematics of chemistry stoichiometry dimensional analysis.pptjami1779
Here is a stoichiometry question I wrote for the given reaction:
If 3.25 grams of barium chloride are available to react, how many grams of barium sulfate can be produced?
Chemistry is the study of matter, its properties, and the changes it undergoes. Matter is anything that has mass and takes up space, and is composed of atoms. Atoms are the building blocks of matter and each element is made of the same type of atom. Compounds are made of two or more different elements chemically bonded together. Mixtures contain two or more substances mixed but not chemically combined. Measurements in chemistry use significant figures and units to accurately quantify properties and changes in matter.
Chemistry is the study of matter, its properties, and the changes it undergoes. Matter is anything that has mass and takes up space, and is composed of atoms. Atoms are the building blocks of matter and each element is made of the same type of atom. Compounds are made of two or more different elements chemically bonded together. Mixtures contain two or more substances mixed but not chemically combined. Measurements in chemistry use significant figures and the SI system of units including meters, grams, and liters.
This document provides an overview of chemistry concepts including:
- Chemistry is the study of matter and its properties, covering topics like health, energy, materials, food and more.
- Matter is anything that has mass and takes up space, and can exist as elements, compounds and mixtures.
- Chemical and physical changes alter substances in different ways. The document also introduces concepts such as states of matter, properties of matter, units of measurement, and dimensional analysis.
This document provides an overview of chemistry concepts including:
1. Chemistry is the study of matter and the changes it undergoes. The scientific method uses a systematic approach involving hypotheses, experiments, and analysis.
2. Matter can exist as elements, compounds, mixtures, and in three main states - solids, liquids, and gases. Chemical and physical changes alter substances in different ways.
3. The study of chemistry incorporates macroscopic observations and measurements as well as analysis at the microscopic level of atoms and molecules. Significant figures, units, and mathematical representations are important tools in chemistry.
- Physical changes do not alter the composition or identity of a substance, while chemical changes do alter the composition or identity of one or more substances.
- Extensive properties depend on amount, while intensive properties do not.
- Mixtures can be separated based on differences in their physical properties, such as filtering solids from liquids, distilling liquids based on differing boiling points, and chromatography.
A physical change alters a substance without changing its chemical identity. During a physical change, no new substance is created and no new chemical bonds form. Examples of physical changes include phase changes like melting, freezing, and vaporization, as well as dissolving and mixing substances that do not undergo chemical reactions.
Chemistry : The Study of change chapter 1RestinaBemis2
This document provides an overview of chemistry and some key concepts in the field. It discusses how chemistry relates to areas like health, energy, materials and technology. It also defines important terms like elements, compounds, mixtures, and the three states of matter. Several examples are given to illustrate states of matter and other concepts. Measurement units and significant figures are explained. The scientific method and types of chemical changes are defined. Dimensional analysis is introduced as a method for solving problems involving unit conversions.
This document provides an overview of chemistry as a science and introduces some key concepts. It discusses how chemistry relates to important areas like health, energy, materials, food and agriculture. The document then defines some basic chemistry terms including matter, elements, compounds, mixtures, physical and chemical changes, states of matter, properties of matter and units of measurement. It also introduces scientific notation and significant figures as well as methods for calculations.
This document discusses measurement and units in science. It begins by defining measurement as reading tools like watches, scales, and thermometers. Standards of measurement are compared to a standard unit using tools. The metric system and SI units are introduced, with prefixes and conversions between units. Equalities show the same measurement in different units. Conversion factors relate different units, and steps for unit conversions in problems are outlined.
This document discusses scientific measurement and units. It covers accuracy, precision, and error in measurements. It introduces the International System of Units (SI) including the base units for length, volume, mass, temperature, and energy. It discusses significant figures and proper handling of calculations and conversions between units using dimensional analysis and conversion factors.
Here are the steps to write a number in standard form:
1. Locate the decimal point in the number.
2. Move the decimal point so that the number is greater than or equal to 1 but less than 10.
3. Count how many places the decimal was moved. If it was moved to the left, the exponent is positive. If it was moved to the right, the exponent is negative.
4. Write the number as the coefficient (the number with 1-9) and 10 with the exponent determined in step 3.
For example:
0.00045 would be written as 4.5 × 10-4
Since the decimal was moved 3 places to the right,
This document provides an overview of basic chemistry concepts. It discusses the following key points in 3 sentences or less:
- Chemistry is the study of matter and the changes it undergoes. Matter can exist in solid, liquid, or gas states. A substance has a definite composition while a mixture combines two or more substances.
- An element is a substance that cannot be broken down further, with over 100 known elements. Compounds are formed from chemical combinations of elements. Physical changes do not alter substance composition while chemical changes do.
- Measurements in chemistry rely on devices like rulers, balances, and thermometers. The standard metric units and prefixes like milli and kilo are used to quantify measurements, properties
Chemistry is the study of matter and the changes it undergoes. Matter has mass and takes up space, and can be either elements or compounds. Elements are pure substances made of one type of atom, while compounds contain two or more elements chemically bonded together. Properties of matter include physical properties that can be observed without changing its composition, and chemical properties that involve its reactivity. Energy is the ability to do work or cause change and can exist in different forms like kinetic, potential, chemical, and heat energy. Heat is the transfer of energy between a system and its surroundings due to a temperature difference. The amount of heat required to change a substance's temperature can be calculated using the formula Q=mcΔT, where
Capítulos 1 y 2 del libro de química de changyesu90uy
This document provides an overview of the development of atomic theory and models of the atom. It discusses key discoveries and experiments including:
- Dalton's atomic theory from 1808 that proposed atoms as fundamental particles and that elements are composed of unique atoms.
- J.J. Thomson's discovery in 1906 that the cathode rays were composed of negatively charged particles (electrons) much lighter than atoms.
- Rutherford's gold foil experiment from 1911 that showed the positive charge and most of the mass of atoms are concentrated in a very small nucleus.
- Chadwick's discovery of the neutron in 1932, which has no charge and a mass similar to protons.
- The modern definitions of atomic number as
This document provides an overview of key concepts in chemistry including the scientific method, properties of matter, states of matter, measurement, and significant figures. Some key points:
- Chemistry is the study of matter, its properties, and the changes it undergoes. The scientific method is used to systematically discover new information through observation, questioning, pattern recognition, experimentation, and summarizing data.
- Matter can be classified by its physical and chemical properties as well as its state - solid, liquid, or gas. Properties include things like color, hardness, and flammability. Changes can be physical, changing a state without altering composition, or chemical, involving changes to composition.
- The metric system is the
This document provides an overview of key concepts from Chapter 3 on scientific measurement, including:
1) It discusses the importance of measurements and units in science, introducing the International System of Units (SI) with base units like meters, kilograms, and seconds.
2) It covers the concepts of accuracy, precision, and errors in measurement, as well as significant figures and proper reporting of measurements.
3) The document outlines methods for unit conversion using dimensional analysis and conversion factors to solve multi-step problems.
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This document discusses measurement, units, accuracy, precision, and density. It contains examples of measuring length in meters, centimeters, and millimeters. It defines accuracy as closeness to a known value and precision as closeness between repeated measurements. Significant figures refer to the digits measured plus one estimated digit used in calculations and rounding. The metric system base units and prefixes like kilo and centi are presented. Density is defined as mass per unit volume and examples show how it can be used to solve problems by setting up ratios or using it as a conversion factor.
This document provides an overview of a science unit on living vs. non-living things and measurement. It includes objectives, activities, and instructions for students. They will identify characteristics of living things, needs for survival, complete a poster comparing living and non-living objects, and learn to use tools like thermometers and graduated cylinders to take measurements in metrics. Students are introduced to key scientific concepts like observations, inferences, predictions, and the scientific method to design experiments and analyze data. Safety procedures are also outlined for laboratory work.
The document discusses scientific measurement and units. It covers accuracy, precision, and significant figures when making measurements. Conversion factors allow measurements to be converted between different units through multiplication. Dimensional analysis uses the units of measurements to solve conversion problems by breaking them into steps. Complex problems are best solved by breaking them into manageable parts.
This document provides an overview of scientific measurement and units covered in a general chemistry course. It discusses the metric system of units used in science including the SI base units. It also covers scientific notation, significant figures, units of temperature, density, specific gravity, and heat measurement.
This presentation discusses Contoso's goals for the next quarter, including synergizing scalable e-commerce, disseminating standardized metrics, coordinating e-business applications, and deploying strategic networks. The presentation outlines Contoso's areas of growth in B2B supply chain, ROI, and e-commerce. It then provides a timeline for the product launch plan and areas of focus on B2B market scenarios and cloud-based opportunities.
This PowerPoint presentation covers various topics and includes an agenda, introduction, topic one with a chart and table, quotes, a team page, timeline, tips on using PowerPoint, and a concluding thank you slide. The presentation teaches how to create and share presentations using PowerPoint across devices by adding text, images, videos and saving to OneDrive for access on a computer, tablet or phone.
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This document provides an overview of chemistry concepts including:
- Chemistry is the study of matter and its properties, covering topics like health, energy, materials, food and more.
- Matter is anything that has mass and takes up space, and can exist as elements, compounds and mixtures.
- Chemical and physical changes alter substances in different ways. The document also introduces concepts such as states of matter, properties of matter, units of measurement, and dimensional analysis.
This document provides an overview of chemistry concepts including:
1. Chemistry is the study of matter and the changes it undergoes. The scientific method uses a systematic approach involving hypotheses, experiments, and analysis.
2. Matter can exist as elements, compounds, mixtures, and in three main states - solids, liquids, and gases. Chemical and physical changes alter substances in different ways.
3. The study of chemistry incorporates macroscopic observations and measurements as well as analysis at the microscopic level of atoms and molecules. Significant figures, units, and mathematical representations are important tools in chemistry.
- Physical changes do not alter the composition or identity of a substance, while chemical changes do alter the composition or identity of one or more substances.
- Extensive properties depend on amount, while intensive properties do not.
- Mixtures can be separated based on differences in their physical properties, such as filtering solids from liquids, distilling liquids based on differing boiling points, and chromatography.
A physical change alters a substance without changing its chemical identity. During a physical change, no new substance is created and no new chemical bonds form. Examples of physical changes include phase changes like melting, freezing, and vaporization, as well as dissolving and mixing substances that do not undergo chemical reactions.
Chemistry : The Study of change chapter 1RestinaBemis2
This document provides an overview of chemistry and some key concepts in the field. It discusses how chemistry relates to areas like health, energy, materials and technology. It also defines important terms like elements, compounds, mixtures, and the three states of matter. Several examples are given to illustrate states of matter and other concepts. Measurement units and significant figures are explained. The scientific method and types of chemical changes are defined. Dimensional analysis is introduced as a method for solving problems involving unit conversions.
This document provides an overview of chemistry as a science and introduces some key concepts. It discusses how chemistry relates to important areas like health, energy, materials, food and agriculture. The document then defines some basic chemistry terms including matter, elements, compounds, mixtures, physical and chemical changes, states of matter, properties of matter and units of measurement. It also introduces scientific notation and significant figures as well as methods for calculations.
This document discusses measurement and units in science. It begins by defining measurement as reading tools like watches, scales, and thermometers. Standards of measurement are compared to a standard unit using tools. The metric system and SI units are introduced, with prefixes and conversions between units. Equalities show the same measurement in different units. Conversion factors relate different units, and steps for unit conversions in problems are outlined.
This document discusses scientific measurement and units. It covers accuracy, precision, and error in measurements. It introduces the International System of Units (SI) including the base units for length, volume, mass, temperature, and energy. It discusses significant figures and proper handling of calculations and conversions between units using dimensional analysis and conversion factors.
Here are the steps to write a number in standard form:
1. Locate the decimal point in the number.
2. Move the decimal point so that the number is greater than or equal to 1 but less than 10.
3. Count how many places the decimal was moved. If it was moved to the left, the exponent is positive. If it was moved to the right, the exponent is negative.
4. Write the number as the coefficient (the number with 1-9) and 10 with the exponent determined in step 3.
For example:
0.00045 would be written as 4.5 × 10-4
Since the decimal was moved 3 places to the right,
This document provides an overview of basic chemistry concepts. It discusses the following key points in 3 sentences or less:
- Chemistry is the study of matter and the changes it undergoes. Matter can exist in solid, liquid, or gas states. A substance has a definite composition while a mixture combines two or more substances.
- An element is a substance that cannot be broken down further, with over 100 known elements. Compounds are formed from chemical combinations of elements. Physical changes do not alter substance composition while chemical changes do.
- Measurements in chemistry rely on devices like rulers, balances, and thermometers. The standard metric units and prefixes like milli and kilo are used to quantify measurements, properties
Chemistry is the study of matter and the changes it undergoes. Matter has mass and takes up space, and can be either elements or compounds. Elements are pure substances made of one type of atom, while compounds contain two or more elements chemically bonded together. Properties of matter include physical properties that can be observed without changing its composition, and chemical properties that involve its reactivity. Energy is the ability to do work or cause change and can exist in different forms like kinetic, potential, chemical, and heat energy. Heat is the transfer of energy between a system and its surroundings due to a temperature difference. The amount of heat required to change a substance's temperature can be calculated using the formula Q=mcΔT, where
Capítulos 1 y 2 del libro de química de changyesu90uy
This document provides an overview of the development of atomic theory and models of the atom. It discusses key discoveries and experiments including:
- Dalton's atomic theory from 1808 that proposed atoms as fundamental particles and that elements are composed of unique atoms.
- J.J. Thomson's discovery in 1906 that the cathode rays were composed of negatively charged particles (electrons) much lighter than atoms.
- Rutherford's gold foil experiment from 1911 that showed the positive charge and most of the mass of atoms are concentrated in a very small nucleus.
- Chadwick's discovery of the neutron in 1932, which has no charge and a mass similar to protons.
- The modern definitions of atomic number as
This document provides an overview of key concepts in chemistry including the scientific method, properties of matter, states of matter, measurement, and significant figures. Some key points:
- Chemistry is the study of matter, its properties, and the changes it undergoes. The scientific method is used to systematically discover new information through observation, questioning, pattern recognition, experimentation, and summarizing data.
- Matter can be classified by its physical and chemical properties as well as its state - solid, liquid, or gas. Properties include things like color, hardness, and flammability. Changes can be physical, changing a state without altering composition, or chemical, involving changes to composition.
- The metric system is the
This document provides an overview of key concepts from Chapter 3 on scientific measurement, including:
1) It discusses the importance of measurements and units in science, introducing the International System of Units (SI) with base units like meters, kilograms, and seconds.
2) It covers the concepts of accuracy, precision, and errors in measurement, as well as significant figures and proper reporting of measurements.
3) The document outlines methods for unit conversion using dimensional analysis and conversion factors to solve multi-step problems.
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This document discusses measurement, units, accuracy, precision, and density. It contains examples of measuring length in meters, centimeters, and millimeters. It defines accuracy as closeness to a known value and precision as closeness between repeated measurements. Significant figures refer to the digits measured plus one estimated digit used in calculations and rounding. The metric system base units and prefixes like kilo and centi are presented. Density is defined as mass per unit volume and examples show how it can be used to solve problems by setting up ratios or using it as a conversion factor.
This document provides an overview of a science unit on living vs. non-living things and measurement. It includes objectives, activities, and instructions for students. They will identify characteristics of living things, needs for survival, complete a poster comparing living and non-living objects, and learn to use tools like thermometers and graduated cylinders to take measurements in metrics. Students are introduced to key scientific concepts like observations, inferences, predictions, and the scientific method to design experiments and analyze data. Safety procedures are also outlined for laboratory work.
The document discusses scientific measurement and units. It covers accuracy, precision, and significant figures when making measurements. Conversion factors allow measurements to be converted between different units through multiplication. Dimensional analysis uses the units of measurements to solve conversion problems by breaking them into steps. Complex problems are best solved by breaking them into manageable parts.
This document provides an overview of scientific measurement and units covered in a general chemistry course. It discusses the metric system of units used in science including the SI base units. It also covers scientific notation, significant figures, units of temperature, density, specific gravity, and heat measurement.
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The document outlines a travel timeline over 4 weeks, visiting North, Utah, Arizona, and California. It details activities like going to a sushi restaurant, pizza place, farmers market, and enjoying macaroons. The timeline shows plans for each day of the week, from Sunday to Friday, with various to-do items and locations mentioned.
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Biosensors convert a biochemical recognition event into a measurable signal and consist of a biological probe and physical detector. There are several types including enzyme-based, immunosensors, and piezoelectric biosensors. Lab-on-chip technology integrates laboratory functions onto a small chip and contains microchannels to flow liquid samples along with integrated measuring components. Examples of lab-on-chip applications described are ones that can detect Ebola virus from a blood sample in 30 minutes and detect HIV using CD4+ cell numbers and magnetophoresis from 10 microliters of whole blood in 20 minutes. Organ-on-chip technology aims to mimic organ behaviors for medical research purposes.
Chloramphenicol was the first antibiotic to be manufactured synthetically for clinical use. It inhibits bacterial protein synthesis by binding to the 50S ribosomal subunit. While broad-spectrum, it carries risks of bone marrow toxicity in humans. Safer derivatives like thiamphenicol and florfenicol were later developed.
Chloramphenicol is a broad-spectrum antibiotic that inhibits bacterial protein synthesis. It binds reversibly to the 50S subunit of bacterial ribosomes, blocking the formation of peptide bonds between amino acids. While effective against many gram-positive and gram-negative bacteria, its use is now reserved for life-threatening infections due to risks of bone marrow suppression and gray baby syndrome in neonates. Proper dosing and alternative antibiotics are preferred whenever possible due to these toxicities.
This document discusses doxycycline, a broad-spectrum antibiotic derived from tetracycline. It inhibits protein synthesis by reversibly binding to the 30S subunit of bacteria to block aminoacyl-tRNA binding. It has activity against many gram-positive and gram-negative bacteria. Doxycycline is used to treat infections caused by Mycoplasma pneumoniae, Rickettsiae, Chlamydia, Vibrio cholerae, Bacillus anthracis, and spirochetes. Adverse effects include gastrointestinal issues, tooth discoloration in children, and photosensitization. It is contraindicated in pregnancy, infants, and those with hypersensitivity.
This document provides an introduction to computational quantum chemistry. It defines computational chemistry as using mathematical approximations and computer programs to solve chemical problems based on quantum mechanics. Specifically, computational quantum chemistry focuses on solving the Schrödinger equation for molecular systems using approximations like the Born-Oppenheimer approximation. It discusses how computational methods can be used to calculate various molecular properties and motivates the need for approximations due to the inability to exactly solve the Schrödinger equation for complex molecules. The document then provides an overview of common computational methods like Hartree-Fock, configuration interaction, Møller-Plesset perturbation theory, and coupled cluster theory.
Computational chemistry uses numerical simulations based on the laws of physics to model chemical structures and reactions. There are different types of computational models of varying accuracy and computational cost, including molecular mechanics, semi-empirical, ab initio, and density functional theory methods. The accuracy of calculations also depends on the basis set used to describe molecular orbitals. Computational chemistry has become an important tool for characterizing nanomaterials.
The document discusses key concepts in chemistry including the scientific method, atomic theory, and the classification of matter. It explains that chemistry uses the scientific method to study matter and its transformations. Matter is anything that has mass and takes up space, and can be classified as elements, compounds, or mixtures. Elements are substances made of only one type of atom, while compounds are made of two or more elements chemically bonded together. Mixtures can be either homogeneous, with consistent properties throughout, or heterogeneous, having distinct parts with different properties. Chemical and physical changes that matter undergoes are also described.
The document provides an introduction to computational chemistry methods, including ab initio, semi-empirical, and density functional theory approaches. It outlines the central theme of relating molecular structure, dynamics, and function through computational modeling. Example applications include modeling small molecules, proteins, crystals and surfaces across various scales from quantum to molecular mechanical methods. Hands-on exercises are included to provide experience with computational chemistry techniques.
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
The simplified electron and muon model, Oscillating Spacetime: The Foundation...RitikBhardwaj56
Discover the Simplified Electron and Muon Model: A New Wave-Based Approach to Understanding Particles delves into a groundbreaking theory that presents electrons and muons as rotating soliton waves within oscillating spacetime. Geared towards students, researchers, and science buffs, this book breaks down complex ideas into simple explanations. It covers topics such as electron waves, temporal dynamics, and the implications of this model on particle physics. With clear illustrations and easy-to-follow explanations, readers will gain a new outlook on the universe's fundamental nature.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
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Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
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This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
2. 2
1.1 Chemistry—The Science of Everyday
Experience
•Chemistry is the study of matter—its composition,
properties, and transformations.
•Matter is anything that has mass and takes up volume.
•Matter can
be:
3. 3
1.2 States of Matter
The Solid State:
• A solid has a definite volume.
• It maintains its shape regardless
of its container.
• Solid particles lie close together
in a regular pattern.
4. 4
1.2 States of Matter
The Liquid State:
• A liquid has a definite volume.
• It takes the shape of its
container.
• Liquid particles are close together
but can move past one another.
5. 5
1.2 States of Matter
The Gas State:
• A gas has no definite shape;
it assumes the shape of its
container.
• It has no definite volume;
it assumes the volume of its
container.
• Gas particles are very far apart
and move around randomly.
6. 6
1.2 States of Matter
Physical properties can be observed or measured
without changing the composition of the material.
•boiling point
•melting point
•solubility
•color
•odor
•state of matter
7. 7
• A physical change alters the material without
changing its composition.
1.2 States of Matter
• Physical changes will be covered in more detail
in Chapter 7.
8. 8
• Chemical properties determine how a
substance can be converted into another
substance.
• Chemical change is the chemical reaction that
converts one substance into another
(Chapters 5 and 6).
1.2 States of Matter
9. 9
1.3 Classification of Matter
• A pure substance is composed of only a
single component (atom or molecule).
• It has a constant composition, regardless of
sample size or origin of sample.
• It cannot be broken down to other pure
substances by a physical change.
I. Pure Substances
All matter can be classified as either a pure substance
or a mixture.
10. 10
•Table sugar (C12H22O11) and water (H2O) are both
pure substances:
1.3 Classification of Matter
I. Pure Substances
All matter can be classified as either a pure substance
or a mixture.
11. 11
1.3 Classification of Matter
II. Mixtures
• Mixtures are composed of more than one
component.
• They can have varying composition (any
combination of solid, liquid, and gas).
• Mixtures can be separated into their components
by a physical process.
All matter can be classified as either a pure substance
or a mixture.
12. 12
1.3 Classification of Matter
• Sugar dissolved in water is a mixture.
II. Mixtures
All matter can be classified as either a pure substance
or a mixture.
13. 13
I. An element is a pure substance that cannot be
broken down by a chemical change.
1.3 Classification of Matter
A pure substance is classified as an element or a
compound.
14. 14
II. A compound is a pure substance formed by
chemically joining two or more elements.
1.3 Classification of Matter
A pure substance is classified as an element or a
compound.
16. 16
• The number is meaningless without the unit.
1.4 Measurement
proper aspirin dosage = 325 (milligrams or pounds?)
a fast time for the 100-meter dash = 10.00 (seconds
or days?)
• Every measurement is composed of a number
and a unit.
Examples:
17. 17
Each type of measurement has a base unit in the
metric system..
1.4 Measurement
A. The Metric System
18. 18
• Other units are related to the base unit by a power of 10.
1.4 Measurement
A. The Metric System
• The prefix of the unit name indicates if the unit is larger
or smaller than the base unit.
19. 19
1 kilometer (km) = 1,000 meters (m)
1 km = 1,000 m
1 millimeter (mm) = 0.001 meters (m)
1 mm = 0.001 m
1 centimeter (cm) = 0.01 meters (m)
1 cm = 0.01 m
1.4 Measurement
B. Measuring Length
• The base unit of length is the meter (m).
20. 20
• Mass is a measure of the amount of matter in an
object.
• Weight is the force that matter feels due to gravity.
1 kilogram (kg) = 1,000 grams (g)
1 kg = 1,000 g
1 milligram (mg) = 0.001 grams (g)
1 mg = 0.001 g
1.4 Measurement
C. Measuring Mass
• The base unit of mass is the gram (g).
21. 21
1 kiloliter (kL) = 1,000 liters (L)
1 kL = 1,000 L
1 milliliter (mL) = 0.001 liters (L)
1 mL = 0.001 L
Volume = Length x Width x Height
= cm x cm x cm
= cm3
1 mL = 1 cm3 = 1 cc
1.4 Measurement
D. Measuring Volume
• The base unit of volume is the liter (L).
23. 23
An exact number results from counting objects or is
part of a definition.
•10 fingers
•10 toes
•1 meter = 100 centimeters
An inexact number results from a measurement or
observation and contains some uncertainty.
•15.3 cm
•1000.8 g
•0.0034 mL
1.5 Significant Figures
24. 24
Significant figures are all the digits in a measured
number including one estimated digit.
All nonzero digits are always significant.
3 sig. figures 6 sig. figures
65.2 g 255.345 g
1.5 Significant Figures
A. Determining Significant Figures
65.2 g 255.345 g
25. 25
3 sig. figures
Rule 1: A zero counts as a significant figure when
it occurs:
•between two nonzero digits
5 sig. figures
•at the end of a number with a decimal place
29.05 g
4 sig. figures
1.0087 mL
29.05 g 1.0087 mL
3.7500
cm
5 sig. figures
620. lb
3.7500
cm
620. lb
1.5 Significant Figures
A. Determining Significant Figures
Rules for Zero:
26. 26
Rule 2: A zero does not count as a significant figure
when it occurs:
5 sig. figures
•at the beginning of a number
1 sig. figure
•at the end of a number that does not have a decimal
0.00245
mg
0.008 mL
3 sig. figures
0.00245
mg
0.008 mL
2570
m
1245500
m
3 sig. figures
2570
m
1245500
m
1.5 Significant Figures
A. Determining Significant Figures
Rules for Zero:
27. 27
351.2 miles
5.5 hour
= 63.854545
miles hour
351.2 miles
5.5 hour
4 sig. figures
2 sig. figures Answer must have
2 sig. figures.
The answer has the same number of significant figures
as the original number with the fewest significant
figures.
1.5 Significant Figures
B. Rules for Multiplication and Division
28. 28
63.854545
miles
to be retained to be dropped
first digit to be dropped
hour
63.854545
If the first digit
to be dropped is: Then:
•between 0 and 4 •drop it and all remaining digits
•between 5 and 9 •round up the last digit
to be retained by adding 1
=
2 sig. figures
Answer
1.5 Significant Figures
B. Rules for Multiplication and Division
64 miles
hour
30. 30
The answer has the same number of decimal places
as the original number with the fewest decimal places.
10.11 kg
3.6 kg
6.51 kg
10.11 kg
3.6 kg
2 decimal places
1 decimal place
answer must have
1 decimal place
= 6.5 kg final answer
1 decimal place
1.5 Significant Figures
C. Rules for Addition and Subtraction
31. 31
y x 10x
Coefficient:
A number between
1 and 10.
y x 10x Exponent:
Any positive
or negative
whole number.
In scientific notation, a number is written
as:
1.6 Scientific Notation
32. 32
HOW TO Convert a Standard Number to Scientific Notation
Example
Step [1]
Step [2]
Convert these numbers to scientific notation.
2,50
0
0.03
6
Move the decimal point to give a number
between 1 and 10.
250
0
0.03
6
Multiply the result by 10x, where
x = number of places the decimal was moved.
•move decimal
left,
x is positive
•move decimal
right,
x is negative
2.5 x 103 3.6 x 10−2
1.6 Scientific Notation
33. 33
•When the exponent x is positive, move the decimal
point x places to the right.
2.80 x 10–2 =
2.800 x 102 =
1.6 Scientific Notation
Converting a Number in Scientific Notation
to a Standard Number
•When the exponent x is negative, move the decimal
point x places to the left.
280.0
0.0280
34. 34
• Conversion factor: A term that converts a quantity in
one unit to a quantity in another unit.
• Conversion factors are usually written as
equalities.
2.20 lb = 1 kg
• To use them, they must be written as fractions.
original
quantity
conversion factor
desired
quantity
x =
1.7 Problem Solving Using
Conversion Factors
A. Conversion Factors
2.20 lb
1 kg
or 1 kg
2.20 lb
35. 35
• If a unit appears in the numerator in one term and
the denominator in another term, the units cancel.
• The goal in setting up a problem is to make sure all
unwanted units cancel.
To convert 130 lb into kilograms:
130 lb x conversion factor = ? kg
original
quantity
desired
quantity
1.7 Problem Solving Using
Conversion Factors
B. Solving a Problem Using One Conversion Factor
36. 36
or
2.20 lb
1 kg
1 kg
2.20 lb
130 lb x
= 59 kg
Answer
2 sig. figures
•The bottom conversion factor has
the original unit in the denominator.
•The unwanted unit lb cancels.
•The desired unit kg does not cancel.
1.7 Problem Solving Using
Conversion Factors
B. Solving a Problem Using One Conversion Factor
37. 37
HOW TO Solve a Problem Using Conversion Factors
Example
How many grams of aspirin are in a 325-mg
tablet?
Step [1]
Identify the original quantity and the desired
quantity, including units.
original quantity desired quantity
325 mg ? g
1.7 Problem Solving Using
Conversion Factors
38. 38
Step [2] Write out the conversion factor(s) needed
to solve the problem.
1 g = 1000 mg
HOW TO Solve a Problem Using Conversion Factors
This can be written as two possible fractions:
or
Choose this factor to
cancel the unwanted
unit, mg.
1000 mg
1g
1 g
1000 mg
1.7 Problem Solving Using
Conversion Factors
39. 39
Step [3]
HOW TO Solve a Problem Using Conversion Factors
Set up and solve the problem.
325 mg x 1 g
1000 mg
= 0.325 g
Step [4]
Write the answer with the correct number
of significant figures.
Unwanted unit
cancels
325 mg 0.325 g
3 sig. figures
3 sig. figures
1.7 Problem Solving Using
Conversion Factors
40. Always arrange the factors so that the denominator in
one term cancels the numerator in the preceding term.
How many liters are in 1.0 pint?
2 pints = 1 quart 1.06 quarts = 1 liter
•Two conversion factors are needed:
1.0 pint
original quantity
? L
desired quantity
1.7 Problem Solving Using
Conversion Factors
C. Solving a Problem Using Two or More Conversion Factors
2 pt
1 qt
1 qt
2 pt
or 1.06 qt
1 L
1 L
1.06 qt
or
First, cancel pt. Then, cancel qt.
41. 41
•Set up the problem and solve:
1.0 pt x 1 qt
2 pt
x 1 L
1.06 qt
= 0.471698113
L
1.0 pt
2 sig. figures
0.47 L
2 sig. figures
•Write the answer with the correct number of
significant figures.
1.7 Problem Solving Using
Conversion Factors
C. Solving a Problem Using Two or More Conversion Factors
42. 42
1.9 Temperature
• Temperature is a measure of how hot or cold
an object is.
1. Degrees Fahrenheit (oF)
2. Degrees Celsius (oC)
3. Kelvin (K)
• Three temperature scales are used:
To convert from oC to oF: To convert from oF to oC:
oF = 1.8(oC) + 32
oC = oF − 32
1.8
To convert from oC to K:
K = oC + 273 oC = K − 273
To convert from K to oC:
44. 44
1.10 Density and Specific Gravity
A. Density
density =
mass (g)
volume (mL or cc)
Density: A physical property that relates the mass of
a substance to its volume.
To convert volume (mL)
to mass (g):
To convert mass (g)
to volume (mL):
mL x
g
mL
= g g x
mL
g
= mL
density inverse of density
45. 45
1.10 Density and Specific Gravity
A. Density
•If the density of acetic acid is 1.05 g/mL, what is
the volume of 5.0 grams of acetic acid?
5.0 g
original quantity
? mL
desired quantity
•Density is the conversion factor, and can be
written two ways:
1.05 g
1 mL
1 mL
1.05 g
Choose the inverse density
to cancel the unwanted unit, g.
Example:
46. 46
1.10 Density and Specific Gravity
A. Density
•Set up and solve the problem:
5.0 g x 1 mL
1.05 g
= 4.761904762 mL
•Write the final answer with the correct number
of significant figures.
5.0 g
2 sig. figures
4.8 mL
2 sig. figures
Unwanted unit
cancels
47. 47
1.10 Density and Specific Gravity
B. Specific Gravity
Specific gravity: A quantity that compares the density
of a substance with the density of water at the
same temperature.
specific gravity = density of a substance (g/mL)
density of water (g/mL)
•The units of the numerator (g/mL) cancel the
units of the denominator (g/mL).
•The specific gravity of a substance is equal to its
density, but contains no units.