Elements, isotops and calculating the relative atomic mass ppt
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The document discusses elements and isotopes. It aims to explain what makes elements different from each other, how isotopes of the same element differ in their number of neutrons, and how to calculate the atomic mass of an element. Students are asked to identify the three types of subatomic particles, provide examples of different elements, discuss isotopes of hydrogen, and learn how to calculate atomic mass.
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The document discusses atomic number, mass number, and isotopes. It defines atomic number as the number of protons in an atom's nucleus, which determines an element's chemical properties. Mass number is the sum of protons and neutrons. Isotopes are atoms with the same number of protons but different neutrons. Isotopes are identified by their mass number written as chemical symbol followed by mass number. The document also discusses molecular formula, empirical formula, and structural formula as examples of chemical formulas that show the number and arrangement of atoms in a compound. It defines molecular, empirical, and structural formulas and provides an example of a structural formula. Finally, it describes ball-and-stick and space-filling molecular models used to
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1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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3) To find an element's electronic configuration, electrons are filled into the lowest available energy shell first.
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1) Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons.
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1. Relative atomic mass (Ar) is the average mass of a single atom of an element compared to 1/12 the mass of one carbon-12 atom.
2. The relative molecular mass (Mr) of a molecule is the sum of the relative atomic masses of all the atoms in the molecule.
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1) Relative atomic mass (RAM) is a measurement of how many times heavier an atom is than 1/12 the mass of one carbon-12 atom. Relative molecular mass (RMM) similarly compares the mass of a molecule to 1/12 the mass of one carbon-12 atom.
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3) The document provides examples of calculating RAM and RMM values for various elements and compounds using the relative scales and given atomic mass values.
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1) Relative atomic mass (RAM) is a measurement of how many times heavier an atom is than 1/12 the mass of one carbon-12 atom. Relative molecular mass (RMM) similarly compares the mass of a molecule to 1/12 the mass of one carbon-12 atom.
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This document provides an overview of atoms, elements, molecules, and compounds. It discusses how everything is made up of atoms, which contain subatomic particles like protons, neutrons, and electrons. Atoms of the same element have the same number of protons. Elements are organized in the periodic table according to their properties and atomic structure. Atoms can bond together to form molecules, which are made of one or more elements. Compounds are molecules made of two or more different elements bonded together. The properties of compounds are different from the individual elements.
Atoms and the periodic table
The document discusses atoms and the periodic table. It describes how atoms are made up of protons, neutrons, and electrons. Elements are organized on the periodic table based on their atomic structure. Each element has a unique atomic symbol and atomic mass. Isotopes are variants of the same element that have different numbers of neutrons. Ions are formed when atoms gain or lose electrons, acquiring an electrical charge.
Structure of Atom CBSE Class 9 PPT-2.pptx
This document provides information about the structure of atoms, including:
1. Neutrons are subatomic particles found in atomic nuclei except hydrogen.
2. Electrons fill atomic shells in a step-wise manner according to the 2n^2 rule.
3. An atom's valency is determined by the number of electrons it gains, loses, or shares to achieve an octet in its outer shell.
Structure of matter atoms and molecules
- An atom is the smallest particle of an element that retains the chemical properties of that element. All atoms of the same element are identical.
- Atoms are very small, not visible even under a powerful microscope. Models like the ball-and-stick model are used to represent atoms and molecules.
- Atoms consist of even smaller subatomic particles - protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The number of protons determines the element.
A++ mission 6 notes part i 2012
The document provides information about atoms and the structure of matter in three sections:
1. Atoms are the building blocks of matter and consist of protons, neutrons, and electrons. The arrangement of atoms determines the properties of different types of matter.
2. Atoms can combine to form compounds and molecules through chemical bonds. Compounds have unique properties that differ from their constituent elements.
3. Matter exists in four states - solid, liquid, gas, and plasma. The state depends on how tightly or freely the atoms and molecules are able to move. Solids have a fixed structure while gases spread freely.
Atoms elements
Atoms and elements can combine in many ways to form useful compounds. An element is made of identical atoms, while a compound is formed from two or more elements chemically bonded together. Atoms are the simplest form of an element, with protons and neutrons in the nucleus and electrons orbiting around. The number of protons determines the element, while isotopes of an element differ in their number of neutrons. Electrons are usually contained within atoms but can give electric shocks. Atoms combine in fixed ratios to form molecules, with the molecular mass determined by adding the atomic masses. Large numbers of atoms are measured in moles, with one mole equaling 6.02x1023 units. Elements form ions by gaining or losing
Atomic structure
An atom is composed of a nucleus containing protons and neutrons surrounded by electrons. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons exist outside the nucleus in the electron cloud. The number of protons defines the element and is equal to the atomic number. The total number of protons and neutrons is the mass number. For neutral atoms, the number of electrons equals the number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
Elements, compounds, molecules and subatomic particles
This document defines and describes the basic concepts of elements, compounds, molecules, and subatomic particles. It states that elements are substances made of atoms with the same number of protons, while compounds contain atoms of different elements chemically combined in fixed ratios. Molecules are the smallest units that retain a compound's characteristics. The three main subatomic particles are protons, neutrons, and electrons, which make up atoms. The document also provides examples and properties of these scientific terms.
Atoms and the periodic table
This document discusses the structure of atoms and the periodic table. It explains that atoms are made up of protons, neutrons, and electrons. Elements are organized on the periodic table based on their atomic number. Each element has an atomic symbol. The document also describes isotopes, which are variants of an element with different numbers of neutrons. It defines key terms like atomic mass, mass number, and ions.
11/16/11
The charge of the ion is indicated
by the superscript number after the element
symbol. A positive number means the atom
lost electrons and is positively charged. A
negative number means the atom gained
electrons and is negatively charged.
Model: Na+ Ion
Sodium ion (Na) that lost 1 electron
Charge: +1
Protons: 11
Electrons: 10
Neutrons: 12
Mass: 22.9898
Model this ion in your notebook!
Model: Cl- Ion
Chlorine ion (Cl) that gained 1 electron
Charge: -1
Protons: 17
Electrons: 18
Neutrons: 18
General Biology. LECTURE 2. THE CHEMICAL FOUNDATION OF LIFE.pptx
This document provides an overview of the chemical foundations of life. It discusses that biochemistry is the study of the structures and roles of chemicals in living organisms. The key points made are:
- Life depends on chemistry as living things are composed of chemical elements like carbon, hydrogen, oxygen, nitrogen.
- Atoms are the basic unit of matter and combine to form molecules and chemical compounds. The four most common elements in living things are carbon, hydrogen, oxygen, and nitrogen.
- Isotopes are atoms of the same element that vary in neutron number. There are three isotopes of hydrogen: protium, deuterium, and tritium.
Chapter 2 atomic structure
This document provides an overview of key concepts related to the chemical basis of life, including:
1) Elements are the fundamental forms of matter that cannot be broken down further through normal means. The most common elements in the human body are oxygen, hydrogen, carbon, nitrogen, and calcium.
2) Atoms are made up of subatomic particles including protons, neutrons, and electrons. The number of protons determines the element, while the number of neutrons can vary between isotopes of the same element.
3) Electrons play an important role in how atoms interact, forming ions by gaining or losing electrons or bonding through electron sharing. The organization of the periodic table is based on electron configurations.
Atomic Strc
- Isotopes are atoms of the same element that have different numbers of neutrons. Some isotopes are radioactive while others are non-radioactive.
- Radioactive isotopes can be useful in medical applications like cancer treatment and dating ancient remains, as well as industrial uses like leak detection. Their half-lives determine how long it takes for half of a sample to decay.
- Atoms gain and lose electrons to form ions, and ionic bonds form between oppositely charged ions. Ionic compounds have high melting points and are usually soluble in water.
Chemistry - Chp 4 - Atomic Structure - Notes
The document summarizes key concepts about atomic structure from sections 4.1 through 4.3 of a chemistry textbook chapter. It discusses the early ideas of Democritus and Dalton's atomic theory. It then explains Rutherford's gold foil experiment and the nuclear model of the atom with protons, neutrons, and electrons. The document also defines atomic number and mass number, and distinguishes between elements and isotopes. It describes how atomic mass is calculated based on natural isotope abundances.
Power Notes Atomic Structure 2014b
This document contains information about atomic structure and the periodic table. It begins with a summary of the development of atomic theory from Democritus to Schrodinger. Models of the atom including the plum pudding model, Rutherford's gold foil experiment, the Bohr model, and the wave mechanic model are described. The basic atomic structure of protons, neutrons, and electrons is explained. Isotopes and ions are defined. The document concludes with notes on atomic mass, atomic number, chemical symbols, and the relationship between atomic structure and the periodic table.
Power Notes Atomic Structure 2014c
This document contains information about atomic structure and the periodic table. It begins with a discussion of early atomic theories proposed by scientists like Democritus, Lavoisier, Dalton, Thomson, Rutherford, Bohr, and Schrodinger. It then provides details on the basic atomic structure including the nucleus, protons, neutrons, and electrons. Isotopes and ions are defined. The periodic table is discussed in relation to atomic number, mass number, and atomic mass. Diagrams illustrate hydrogen isotopes and charged hydrogen ions. Homework is assigned to continue working on atomic structure in the next week.
Intro to atoms
This document provides information about atoms including:
- Atoms are the smallest particle into which an element can be divided and still be the same substance.
- Atoms are made up of protons, neutrons, and electrons, with protons and neutrons in the nucleus and electrons orbiting around it.
- The number of protons determines the identity of an element.
- Various exercises and questions are provided to help teach and test understanding of atomic structure and terminology.
Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons. Atoms of the same element have the same atomic number but can have different mass numbers, which is caused by varying numbers of neutrons. Isotopes can be stable or unstable depending on their nucleus - unstable isotopes have different numbers of nucleons (protons and neutrons) in their nucleus, making the mass different and causing instability. Common stable isotopes include carbon-12 and carbon-13, while unstable isotopes include carbon-14 and potassium-40.
identify proton, neutrons and electrons.pptx
An atom is composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons move around the nucleus. The number of protons determines the element, while the number of neutrons can vary, creating isotopes of that element. Isotopes are identified by their isotope notation, which includes the element symbol, mass number (protons + neutrons), and atomic number (protons).
10/15 Review: Atomic Structure
This document provides an overview of an upcoming chemistry class covering atomic structure. The weekly schedule outlines topics to be covered each day, including atomic radius, electronegativity, atomic structure, and a midterm exam on Friday. Students are instructed to sketch the periodic table and label families for homework. The document then reviews atomic structure, including the dense nucleus at the center containing protons and neutrons, and less dense electron shells. Examples are given to calculate protons, neutrons, and electrons in different atoms. Homework assigned is to make a study notecard and complete a review worksheet in preparation for the midterm.
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Elements, compounds, molecules and subatomic particles
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Thematic analysis in qualitative research is a time-consuming and systematic task, typically done using teams. Team members must ground their activities on common understandings of the major concepts underlying the thematic analysis, and define criteria for its development. However, conceptual misunderstandings, equivocations, and lack of adherence to criteria are challenges to the quality and speed of this process. Given the distributed and uncertain nature of this process, we wondered if the tasks in thematic analysis could be supported by readily available artificial intelligence chatbots. Our early efforts point to potential benefits: not just saving time in the coding process but better adherence to criteria and grounding, by increasing triangulation between humans and artificial intelligence. This tutorial will provide a description and demonstration of the process we followed, as two academic researchers, to develop a custom ChatGPT to assist with qualitative coding in the thematic data analysis process of immersive learning accounts in a survey of the academic literature: QUAL-E Immersive Learning Thematic Analysis Helper. In the hands-on time, participants will try out QUAL-E and develop their ideas for their own qualitative coding ChatGPT. Participants that have the paid ChatGPT Plus subscription can create a draft of their assistants. The organizers will provide course materials and slide deck that participants will be able to utilize to continue development of their custom GPT. The paid subscription to ChatGPT Plus is not required to participate in this workshop, just for trying out personal GPTs during it.
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Classification
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The cost of acquiring information by natural selection
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It's based on the first part of this research paper:
The cost of information acquisition by natural selection
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Disclaimer: No one is perfect, so please mind that there might be mistakes and typos.
dtubbenhauer@gmail.com
Corrected slides: dtubbenhauer.com/talks.html
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- 1. Lesson objectives: • Explain what makes one element different from another • Explain how isotopes of an element differ • Calculate the atomic mass of an element
- 2. What makes elements different from each other? Gold Carbon Sodium
- 3. What makes elements different from each other? Q: what were the three types of the subatomic particles?
- 5. What makes elements different from each other? Elements are different from each other, because they have different numbers of electrons.
- 6. Isotopes of given elements Isotopes: are the atoms of an element with different numbers of neutrons. They have the same proton number, but different mass numbers.
- 7. ISOTOPES Hydrogen-1 : It has 1 electron, 0 neutron and 1 proton Draw an electronic configuration for this isotope?
- 8. ISOTOPES Now tell me, how many electrons, neutrons and electrons does: Hydrogen-2 and Hydrogen-3 have? Discuss in pairs! You have one minute
- 9. Calculating the atomic mass