Atomic bbst 1
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1. The document traces the history of atomic models from Dalton's early atomic theory in 1808 to Bohr's refinement of Rutherford's nuclear model in 1913. 2. Key developments included Thomson's discovery of the electron in 1898, Rutherford's gold foil experiment in 1910 which led to the proposal of a nuclear model of the atom, and Bohr's addition of electron orbits to Rutherford's model in 1913. 3. The document also describes the structure of atoms including the numbers and properties of subatomic particles like protons, neutrons, and electrons, as well as how electrons are arranged in shells around the nucleus according to their energy levels.
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Atomic structure
1. The document discusses the history of atomic theory from ancient Greek philosophers to modern scientists like Rutherford and Bohr.
2. Key developments included Dalton's atomic theory, Thomson's discovery of the electron, and Rutherford's gold foil experiment which led him to propose that atoms have a small, dense nucleus.
3. Bohr further refined the model by suggesting that electrons orbit the nucleus in set shells corresponding to specific energy levels.
Atomic Structure
This document discusses the history and structure of the atomic model. It describes early theories from Democritus and Dalton that atoms were indivisible spheres. In the 1890s, Thomson discovered the electron and proposed the "plum pudding" model where electrons were distributed within the atom. Rutherford's gold foil experiment in 1910 showed that the positive charge and mass of atoms were concentrated in a small nucleus. Bohr added to this in 1913 by suggesting that electrons orbit the nucleus in set energy levels or shells. The document then explains atomic structure, including atomic number, mass, and how electrons are arranged in shells around the nucleus.
Atomic Structure
1. The document traces the history of ideas about the atom from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913.
2. In the early 20th century, Rutherford discovered that atoms have a small, dense nucleus through experiments deflecting helium nuclei with gold foil.
3. Bohr then refined Rutherford's model by proposing that electrons orbit the nucleus in set energy levels, like planets orbiting the sun.
Atomic structure
1. The document traces the history of ideas about the atom from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913.
2. In the early 1900s, Rutherford discovered that atoms have a small, dense nucleus through experiments showing some alpha particles rebounding from gold foil.
3. Bohr refined Rutherford's nuclear model by proposing that electrons orbit the nucleus in set energy levels, like planets orbiting the sun. This helped explain atomic structure and properties.
Atomic structure enet
This document discusses the structure of atoms. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and have a mass of 1. Neutrons are neutral with a mass of 1. Electrons are negatively charged with nearly no mass. The number of protons determines the element, while the number of neutrons varies between isotopes of the same element. Examples of hydrogen, helium, lithium, and beryllium atoms are given with their proton, neutron, and electron composition.
2016 Topic 2: Atomic Structure
This document discusses atomic structure and properties. It begins by reviewing the basic atomic model including protons, neutrons, and electrons. It then discusses atomic number, mass number, isotopes, ions, and electron configuration. The document also covers average atomic mass and mass spectrometry. It concludes by discussing the Bohr model of the atom and how this helped explain emission spectra of elements. In summary, the key topics covered are the fundamental particles of atoms, atomic notation, isotopes, ions, electron configuration, and early atomic structure models.
Atomsintro
This self-guided computer activity introduces students to the topic of atoms through interactive lessons and websites. It is divided into two parts, with part one covering the atomic-molecular theory of matter and how scientists gather evidence about atoms through models and indirect observation. Part two discusses the structure of atoms including the nucleus, electrons, and subatomic particles, as well as isotopes and radioactive decay. Students are instructed to complete a study guide as they proceed through the lessons.
the building block ATOMS
this ppt is all about basic working of most basic unit atom. and could enrich your knowledge about atom. and follow me at my instagram
https://www.instagram.com/shantanu_stark/?hl=en
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Atomic structure
1. The document discusses the history of atomic theory from ancient Greek philosophers to modern scientists like Rutherford and Bohr.
2. Key developments included Dalton's atomic theory, Thomson's discovery of the electron, and Rutherford's gold foil experiment which led him to propose that atoms have a small, dense nucleus.
3. Bohr further refined the model by suggesting that electrons orbit the nucleus in set shells corresponding to specific energy levels.
Atomic Structure
This document discusses the history and structure of the atomic model. It describes early theories from Democritus and Dalton that atoms were indivisible spheres. In the 1890s, Thomson discovered the electron and proposed the "plum pudding" model where electrons were distributed within the atom. Rutherford's gold foil experiment in 1910 showed that the positive charge and mass of atoms were concentrated in a small nucleus. Bohr added to this in 1913 by suggesting that electrons orbit the nucleus in set energy levels or shells. The document then explains atomic structure, including atomic number, mass, and how electrons are arranged in shells around the nucleus.
Atomic Structure
1. The document traces the history of ideas about the atom from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913.
2. In the early 20th century, Rutherford discovered that atoms have a small, dense nucleus through experiments deflecting helium nuclei with gold foil.
3. Bohr then refined Rutherford's model by proposing that electrons orbit the nucleus in set energy levels, like planets orbiting the sun.
Atomic structure
1. The document traces the history of ideas about the atom from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913.
2. In the early 1900s, Rutherford discovered that atoms have a small, dense nucleus through experiments showing some alpha particles rebounding from gold foil.
3. Bohr refined Rutherford's nuclear model by proposing that electrons orbit the nucleus in set energy levels, like planets orbiting the sun. This helped explain atomic structure and properties.
Atomic structure enet
This document discusses the structure of atoms. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and have a mass of 1. Neutrons are neutral with a mass of 1. Electrons are negatively charged with nearly no mass. The number of protons determines the element, while the number of neutrons varies between isotopes of the same element. Examples of hydrogen, helium, lithium, and beryllium atoms are given with their proton, neutron, and electron composition.
2016 Topic 2: Atomic Structure
This document discusses atomic structure and properties. It begins by reviewing the basic atomic model including protons, neutrons, and electrons. It then discusses atomic number, mass number, isotopes, ions, and electron configuration. The document also covers average atomic mass and mass spectrometry. It concludes by discussing the Bohr model of the atom and how this helped explain emission spectra of elements. In summary, the key topics covered are the fundamental particles of atoms, atomic notation, isotopes, ions, electron configuration, and early atomic structure models.
Atomsintro
This self-guided computer activity introduces students to the topic of atoms through interactive lessons and websites. It is divided into two parts, with part one covering the atomic-molecular theory of matter and how scientists gather evidence about atoms through models and indirect observation. Part two discusses the structure of atoms including the nucleus, electrons, and subatomic particles, as well as isotopes and radioactive decay. Students are instructed to complete a study guide as they proceed through the lessons.
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The document discusses the development of atomic models and the structure of atoms. It describes early models like the plum pudding model and Rutherford's solar system model. Modern atomic structure consists of protons and neutrons in the nucleus and electrons in shells or orbits around the nucleus. The key properties of subatomic particles like protons, neutrons and electrons are given. Proton number is defined as the number of protons in an atom and nucleon number as the sum of protons and neutrons. Examples are provided to show how to determine the number of protons, neutrons and electrons from the periodic table.
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This document summarizes the development of atomic models by several scientists:
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- Rutherford discovered the nucleus by observing particles bouncing off a thin gold foil. He calculated the nucleus was very small compared to the atom.
- Bohr built on this work by suggesting electrons orbit in specific energy levels or shells, and can jump between shells by gaining or losing energy. Each shell can only contain a fixed number of electrons.
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The document discusses electronic configurations of atoms. It explains that the electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells in its ground state, and can also represent ionized atoms. Many physical and chemical properties correlate to unique electron configurations, especially the valence electrons in the outermost shell. Electrons fill orbitals according to increasing energy levels and subshells in a set order. Orbital diagrams, spdf notation, and noble gas notation are used to represent electron configurations.
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This document discusses electron configuration and the rules that define how electrons are arranged in an atom's orbitals. It explains:
1) There are three main rules that define electron configuration: the Aufbau principle, Pauli exclusion principle, and Hund's rule.
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3) Electron configuration can be represented using orbital diagrams with arrows or electron configuration notation using symbols and superscripts.
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- The Pauli Exclusion Principle states that no two electrons can have the same set of 4 quantum numbers.
- Elements are arranged on the periodic table based on their electron configurations, with groups reflecting which orbitals are being filled.
- A noble gas configuration can be used to abbreviate long electron configurations by writing the nearest noble gas followed by the remaining electrons.
Electron configuration.ppt
Electron configuration refers to the distribution of electrons in an atom's orbitals and energy levels. There are three main principles that determine electron configuration: 1) Electrons have higher energy further from the nucleus and in higher principal quantum shells, 2) Orbitals within a shell have set ordering of energies (s < p < d < f), and 3) Each orbital can hold a maximum of two electrons of opposite spin. The Aufbau principle, Pauli exclusion principle, and Hund's rule further define how electrons fill the orbitals in atoms.
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This document provides an overview of atomic structure and properties. It discusses John Dalton's atomic theory, early atomic models including Thomson's plum pudding model and Rutherford's nuclear model. Later, it describes Bohr's model of electron orbits and different atomic orbitals. The document also defines key atomic properties including atomic number, mass number, and isotopes.
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The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
Electron configuration lecture notes
This document provides information about electron configuration and the principles that define how electrons are arranged in an atom's orbitals. It discusses the ground-state electron configuration as the most stable, lowest-energy arrangement of electrons in an atom. Three main rules that define electron configuration are described as the Aufbau principle, Pauli exclusion principle, and Hund's rule. The document also explains how electron configuration can be written using orbital diagrams or notation, and how the noble gas notation is used.
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The document discusses electronic structure and the periodic table. It explains that electronic configuration describes how electrons are arranged in an atom's orbitals and can be represented using symbols. The periodic table is organized based on the maximum number of electrons that can fill different atomic orbitals. Valence electrons in the outer shell largely determine an element's chemical properties. The document also summarizes periodic trends in atomic size, ionization energy, and electron affinity.
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The document discusses the development of atomic models and the structure of atoms. It describes early models like the plum pudding model and Rutherford's solar system model. Modern atomic structure consists of protons and neutrons in the nucleus and electrons in shells or orbits around the nucleus. The key properties of subatomic particles like protons, neutrons and electrons are given. Proton number is defined as the number of protons in an atom and nucleon number as the sum of protons and neutrons. Examples are provided to show how to determine the number of protons, neutrons and electrons from the periodic table.
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This document summarizes the development of atomic models by several scientists:
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- Rutherford discovered the nucleus by observing particles bouncing off a thin gold foil. He calculated the nucleus was very small compared to the atom.
- Bohr built on this work by suggesting electrons orbit in specific energy levels or shells, and can jump between shells by gaining or losing energy. Each shell can only contain a fixed number of electrons.
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The document summarizes the evolution of atomic models from Dalton's billiard ball model in 1803 to the modern quantum mechanical model. It traces the key discoveries and models of Thomson, Rutherford, Bohr, Schrodinger that led to the understanding that electrons occupy discrete energy levels and orbitals around the nucleus rather than definite orbits, described by quantum numbers. The modern atomic model uses orbitals and quantum mechanics to describe the probability of finding electrons in an atom.
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The document discusses electronic configurations of atoms. It explains that the electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells in its ground state, and can also represent ionized atoms. Many physical and chemical properties correlate to unique electron configurations, especially the valence electrons in the outermost shell. Electrons fill orbitals according to increasing energy levels and subshells in a set order. Orbital diagrams, spdf notation, and noble gas notation are used to represent electron configurations.
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This document discusses electron configuration and the rules that define how electrons are arranged in an atom's orbitals. It explains:
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- Electron configuration describes the arrangement of electrons in an atom's orbitals and energy levels according to 4 quantum numbers.
- The Pauli Exclusion Principle states that no two electrons can have the same set of 4 quantum numbers.
- Elements are arranged on the periodic table based on their electron configurations, with groups reflecting which orbitals are being filled.
- A noble gas configuration can be used to abbreviate long electron configurations by writing the nearest noble gas followed by the remaining electrons.
Electron configuration.ppt
Electron configuration refers to the distribution of electrons in an atom's orbitals and energy levels. There are three main principles that determine electron configuration: 1) Electrons have higher energy further from the nucleus and in higher principal quantum shells, 2) Orbitals within a shell have set ordering of energies (s < p < d < f), and 3) Each orbital can hold a maximum of two electrons of opposite spin. The Aufbau principle, Pauli exclusion principle, and Hund's rule further define how electrons fill the orbitals in atoms.
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This document provides an overview of atomic structure and properties. It discusses John Dalton's atomic theory, early atomic models including Thomson's plum pudding model and Rutherford's nuclear model. Later, it describes Bohr's model of electron orbits and different atomic orbitals. The document also defines key atomic properties including atomic number, mass number, and isotopes.
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The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
Electron configuration lecture notes
This document provides information about electron configuration and the principles that define how electrons are arranged in an atom's orbitals. It discusses the ground-state electron configuration as the most stable, lowest-energy arrangement of electrons in an atom. Three main rules that define electron configuration are described as the Aufbau principle, Pauli exclusion principle, and Hund's rule. The document also explains how electron configuration can be written using orbital diagrams or notation, and how the noble gas notation is used.
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The document discusses the structure of matter at the atomic level. It explains that all matter is made up of atoms, which themselves are made of even smaller particles like protons, neutrons, and electrons. The structure of atoms determines their chemical properties and how they interact. Atoms can bond together through the sharing or transfer of valence electrons in their outer shells.
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The document summarizes the Bohr model of the atom and electronic configuration. It explains that electrons can only occupy certain energy levels or orbits around the nucleus, and that electrons in orbits further from the nucleus require more energy to remove. It also discusses how the ionization energy increases with each subsequent electron removed from atoms and ions. Finally, it introduces how elements are written with their full electron configuration including shells and subshells.
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Atomic structure
1. The document traces the history of atomic theory from Democritus' idea of indivisible atoms in 460 BC to Bohr's refinement of Rutherford's nuclear model in 1913, which proposed that electrons orbit the nucleus in set energy levels.
2. It then explains the structure of atoms, defining protons, neutrons, electrons, and their properties. Atomic number is defined as the number of protons, while atomic mass includes protons and neutrons.
3. The document concludes by explaining how electronic configuration and dot-and-cross diagrams are used to represent the atomic structure and distribution of electrons in shells for different elements.
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1. The document traces the history of ideas about the atom from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913.
2. In the early 1900s, Rutherford discovered that atoms have a small, dense nucleus through experiments showing some alpha particles rebounding from gold foil.
3. Bohr refined Rutherford's nuclear model by proposing that electrons orbit the nucleus in set energy levels, like planets orbiting the sun. This helped explain atomic structure and properties.
Atomic Structure.pptx
The document traces the history of atomic theory from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913. Key developments included Dalton suggesting atoms were tiny spheres in 1808, Thompson discovering the electron in 1898 and proposing the plum pudding model, and Rutherford's gold foil experiment in 1910 leading him to propose that atoms have a small, dense nucleus.
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The document traces the history of atomic theory from Democritus' idea of indivisible atoms in 460 BC to Bohr's model of electrons orbiting the nucleus in 1913. Key developments included Dalton suggesting atoms were tiny spheres in 1808, Thompson discovering the electron in 1898 and proposing the plum pudding model, and Rutherford deducing the nucleus from deflection experiments in 1910. Bohr later refined Rutherford's model by establishing electrons in distinct orbitals around the nucleus.
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Students can download and use it for studying atomic structure.
Atomic structure
The document summarizes the history of the atomic model from ancient Greek philosophers to modern atomic theory. It discusses early atomic theories proposed by Democritus, Dalton, and Thomson. It then covers pivotal experiments and models proposed in the early 20th century, including Rutherford's gold foil experiment, which led him to propose the nuclear model of the atom. The document also discusses Bohr's refinement of adding electron orbits to Rutherford's nuclear model. Finally, it provides explanations of atomic structure including electronic configuration, atomic number, atomic mass, electron shells, and dot and cross diagrams.
Structure Of The Atom - Class 9
1) An atom is made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus.
2) Rutherford's gold foil experiment showed that the mass and positive charge of an atom are concentrated in a small nucleus.
3) Bohr's model improved upon Rutherford's by proposing that electrons can only orbit in discrete, fixed energy levels rather than any path, resolving the issue of electrons radiating energy in orbits.
athe structure of atom class -9th.pdf
The document discusses the structure of the atom. It explains the key discoveries and models that helped reveal the internal structure of atoms, including Thomson's plum pudding model, Rutherford's nuclear model based on his gold foil experiment, and Bohr's model incorporating allowed electron orbits. It describes the subatomic particles - electrons, protons, and neutrons - and how they are arranged in the nucleus and electron shells. The document also discusses concepts like atomic number, mass number, isotopes, valency, and electronic configuration.
L2atomsionsandmolecules 130906000808-
1) The document discusses Dalton's atomic theory and the key discoveries that led to the modern understanding of atomic structure.
2) It describes J.J. Thomson's discovery of electrons in cathode rays and Millikan's oil drop experiment which determined the charge of an electron.
3) Rutherford's gold foil experiment revealed that atoms have a small, dense nucleus containing most of their mass, with electrons in the space around the nucleus.
Atomic Structure Powerpoint Presentation by Computer Careers
Powerpoint Presentation on Atomic Structure by Computer Careers.What is an Atom?ATOMIC STRUCTURE,There are two ways to represent the atomic structure of n element or compound,DOT & CROSS DIAGRAMS and many more ....
Atomicstructureppt 140315053706-phpapp02
This document provides information about atomic structure. It discusses the basic parts of an atom including protons, neutrons, and electrons. Early atomic models proposed by Rutherford and Bohr are described, noting their limitations in explaining experimental observations. The modern quantum mechanical model represents electrons using quantum numbers and wave functions or "fuzzy clouds" to describe atomic orbitals. Electrons occupy different energy levels and sublevels based on their quantum numbers.
Atomic concepts
The document discusses the evolution of atomic theory from ancient Greek concepts to modern atomic theory. It covers key developments including Dalton's atomic theory, the discovery of the electron by J.J. Thompson, Rutherford's gold foil experiment which led to the discovery of the nucleus, and the development of the Bohr model showing electrons orbiting the nucleus in shells. Modern atomic theory incorporates wave-mechanical models and the dual particle-wave nature of electrons.
Structure Of The Atom.pdf notes important
The document provides information on the structure of atoms, including key experiments and models that helped reveal the internal structure of atoms. It discusses J.J. Thomson's cathode ray experiment that discovered electrons, Rutherford's alpha particle scattering experiment that showed atoms have a small, dense nucleus, and Bohr's model of electron orbits around the nucleus. It also covers topics like isotopes, mass number, atomic number, electron configuration, and valency.
Quantum numbers chemisrty
1) The document discusses the topic-structure of an atom and summarizes the key discoveries that led to modern atomic theory, including the discovery of the electron, proton, neutron, and development of atomic models.
2) It describes Michael Faraday's experiments in the 1830s that provided early insights into atomic structure and the discovery of the electron in the 1850s from cathode ray experiments.
3) The document also summarizes Bohr's 1913 model of the hydrogen atom which explained its spectral lines by postulating stable electron orbits, and the development of quantum mechanics and Schrodinger's equation to more fully describe atomic structure.
ch4 structure of an atom.pdf
The document provides information about the structure of atoms. It discusses that atoms are made up of protons, neutrons and electrons. The protons and neutrons are located in the nucleus at the center, while the electrons move around the nucleus. It explains different atomic models proposed by scientists like Thomson, Rutherford and Bohr. It also discusses the distribution of electrons in shells, valency, atomic number and mass number. Isotopes and isobars are defined. In summary, the document outlines the key particles that make up an atom and the various atomic structure models developed over time.
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Atomic Structure Powerpoint Presentation by Computer Careers
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Chemical for consumer
This document discusses several medicinal plants and their uses, including aloe vera for skin issues, garlic for infections and blood pressure, and ginseng for general health. It also lists some types of modern medicines such as antibiotics like penicillin for bacteria, analgesics like aspirin for pain relief, and psychotherapeutic drugs for mental illnesses.
Chapter 5 medicines kumpulan anis(3)
This document discusses different types of medicines. It describes traditional medicines as being derived from plants or animals and potentially toxic to the liver. Modern medicines are manufactured chemicals that can be extracted from plants and animals or be synthetic. Examples of modern medicines include analgesics like paracetamol and aspirin which relieve pain, antibiotics like penicillin which kill bacteria, and psychotherapeutic medicines like antidepressants which treat mental illnesses. Both traditional and modern medicines can have undesirable side effects, so it is important to only take medicines under medical supervision and at the proper dosage.
Soap & detergent che nur nadira
This document discusses soaps and detergents. Soap is made by heating oils or fats with an alkali like sodium hydroxide, which forms salts from the fatty acids. Detergents are made from petroleum raw materials and form salts from alkyl hydrogen sulfate. Both soaps and detergents dissolve in water, with one polar end attracting water and one nonpolar end attracting dirt and oils. Detergents are more effective cleaners, especially in hard water which causes soap to form insoluble scum. Detergents do not form scum in hard water.
Soap & detergent kump syahirah
This document discusses soap and detergents. It defines soap as the salt formed from reacting a fatty acid with an alkali like sodium hydroxide or potassium hydroxide. Detergents are similar but use alkyl hydrogen sulfates instead of fatty acids. The document describes the production processes for soap and detergents which involve saponification and neutralization reactions. It also explains how the hydrophobic and hydrophilic regions of soap and detergent molecules allow them to interact with both water and grease/oil to facilitate cleaning. The effectiveness of soap can be reduced in hard water which causes soap scum, while detergents are more effective cleaners and do not form scums.
Elements in period 3 smkbbst
The document summarizes the elements in period 3 of the periodic table (Na, Mg, Al, Si, P, S, Cl, Ar), their electron configurations, properties, and how those properties change across the period. It notes that atomic radius decreases and electronegativity increases from left to right as nuclear charge increases. Oxides change from basic to acidic. It predicts similar trends in other periods and discusses how semimetals like silicon are used in electronics as semiconductors in devices like diodes and transistors.
Preparing alcohols
This document discusses two methods for preparing alcohols: hydration of alkenes and fermentation. Hydration of alkenes involves adding water to alkenes to produce alcohols, as shown in the equations for ethene and propene. Fermentation uses yeast and sugar to produce ethanol only, through a process where the yeast enzyme zymase breaks down glucose into ethanol and carbon dioxide. The document also covers physical and chemical properties of alcohols such as boiling points, solubility, combustion, dehydration, oxidation, and reaction with sodium.
Naming alcohols
Alcohols are named with the suffix 'ol' and the carbon chain is identified like alkanes but with an 'e' replaced by 'ol', such as ethanol. The position of the hydroxyl group and any alkyl groups attached to the carbon chain are identified by numbers. The hydroxyl group is always given the lowest possible number. Examples show naming various alcohols based on the longest carbon chain, position of the hydroxyl group, and any alkyl groups.
Alcohol
This document discusses the properties and isomerism of alcohols. Alcohols have the general formula CnH2n+1OH and contain a hydroxyl functional group (-OH). The first three members are methanol, ethanol, and propanol. Alcohols are compounds where hydrogen atoms in alkanes are replaced with -OH groups, making them non-hydrocarbon. Alcohol isomerism occurs due to the position of the hydroxyl group or presence of branching alkyl groups, as seen with propanol and butanol isomers.
Sample p2 kimia 2013
The document provides information about the structure of atoms, bonding, boiling and melting points of substances.
It discusses the stability of argon due to its full outer electron shell configuration. Sodium and chlorine atoms form the ionic compound NaCl by sodium donating an electron to form Na+ and chlorine gaining an electron to form Cl-. Ionic bonds form between the oppositely charged ions.
The experiment to determine the empirical formula of copper oxide involves heating copper(II) oxide with hydrogen gas. The mass changes are used to calculate the ratio of atoms in the empirical formula.
Bonds
The document discusses several key concepts in chemistry including:
- Chemical bonding can be covalent, involving the sharing of electron pairs between atoms, or ionic, involving the transfer of electrons from one atom to another. The type of bond formed depends on the electronegativity of the atoms.
- The periodic table arranges elements and allows prediction of elemental properties based on atomic number. Elements in the same group have similar properties.
- Compounds are named based on their composition and bonding type. Ionic compounds involve cation and anion names while covalent compounds use prefixes to denote atom counts.
- Transition metals can form complexes with variable charges that are indicated in names.
Relative atomic mass
This document discusses relative atomic mass and relative molecular mass. It provides examples to calculate these values.
The key points are:
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.
3. Examples are provided to calculate relative atomic masses and relative molecular masses using atomic mass values and molecular formulas. Formulas, atomic masses, and molecular masses are compared to calculate unknown values.
Chemical formulae
The document discusses chemical formulae and how they are used to represent elements and compounds. It provides examples of how to determine the empirical and molecular formula of substances based on experimental data like mass percentages and ratios of elements. Empirical formulae show the simplest whole number ratio of atoms in a compound, while molecular formulae show the actual number of each atom in a molecule of a substance. Percentage composition can also be calculated from the relative atomic masses and molecular formula.
Homologous series
Homologous series are groups of compounds that have similar chemical properties and differ from each other by an additional CH2 group. To be considered homologous, a series must: 1) have members that can be represented by a common chemical formula; 2) have members that differ by 14 amu (-CH2-); 3) have members prepared through the same chemical reaction; and 4) have members that exhibit the same chemical properties. The presence of a common functional group determines the chemical properties within each homologous series.
Combustion of hydrocarbon
1. Hydrocarbons are organic compounds made of only carbon and hydrogen. They can be classified as saturated or unsaturated depending on the bonding between carbon atoms.
2. Saturated hydrocarbons contain only single bonds between carbons, like alkanes. Unsaturated hydrocarbons contain at least one double bond between carbons, like alkenes.
3. Hydrocarbons undergo complete or incomplete combustion with oxygen, producing carbon dioxide, water, and sometimes carbon monoxide or soot depending on the availability of oxygen.
Carbon compound
Carbon has 6 electrons and forms 4 covalent bonds to achieve stability. Methane (CH4) forms when a carbon atom bonds with 4 hydrogen atoms. Ethane (C2H6) forms when 2 carbon atoms bond, with each carbon also bonding to 3 hydrogen atoms. Carbon can form single, double, or triple bonds. Carbon compounds are divided into organic compounds containing carbon-hydrogen bonds, and inorganic compounds lacking carbon-hydrogen bonds.
Alkane
Alkanes are the simplest family of hydrocarbons containing only carbon and hydrogen. They contain only single covalent bonds between carbon atoms and between carbon and hydrogen atoms, making them chemically stable and difficult to break down. Alkanes undergo combustion reactions with oxygen, producing carbon dioxide and water. When enough oxygen is present, complete combustion occurs, but incomplete combustion produces carbon monoxide or soot if oxygen is limited. Larger alkane molecules contain a higher percentage of carbon and are more likely to produce soot when burned. Alkanes can also undergo substitution reactions where halogen atoms replace hydrogen when exposed to ultraviolet light.
Tuition mole exercise revision
This document contains 15 multiple choice questions related to chemistry concepts such as moles, empirical formulas, relative atomic mass, and chemical equations. Specifically:
- Questions 1-5 ask about calculating the number of molecules or mass of substances using values like the Avogadro constant and relative atomic masses.
- Questions 6-10 involve determining empirical formulas from the percentages or relative masses of elements in compounds.
- Questions 11-15 require balancing chemical equations or identifying products of reactions given word equations.
The questions cover a range of foundational chemistry topics and calculations involving moles, masses, empirical formulas and chemical equations.
Concept of mole
1. A mole is defined as the amount of substance containing 6.02 x 1023 particles and can refer to atoms, molecules, or ions.
2. The mole is the unit for quantifying amount of substance, with the symbol "mol".
3. The number of particles in a given number of moles can be calculated by multiplying the moles by Avogadro's number, and the moles for a given number of particles is calculated by dividing the particles by Avogadro's number.
Factors affecting rate of reaction (recovered)
The document discusses how several factors affect the rate of chemical reactions according to collision theory:
1. Increasing the surface area of reactants by decreasing their size increases the rate of reaction by increasing collision frequency.
2. Higher concentrations increase collision frequency by providing more particles in a given volume, likewise increasing the reaction rate.
3. Higher temperatures cause reactants to move faster and collide more frequently, also increasing the reaction rate.
4. Catalysts can lower the activation energy for a reaction, increasing the frequency of effective collisions and thereby accelerating the reaction.
5. For gas reactions, higher pressures compress the gas, providing more particles per volume and thus more collisions and a faster reaction.
Finding instantaneous rate of reaction from a graph
The instantaneous rate of reaction at a particular time can be determined from a graph of products over time. It is equal to the slope of the tangent line drawn at that time point. For example, to find the rate of reaction at 40 seconds from a graph of carbon dioxide volume released over time, the slope of the tangent line at 40 seconds is calculated using the volumes and times of the points straddling it, giving a rate of 1.4 cm3/s.
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Atomic bbst 1
- 2. HISTORY OF THE ATOM 1 1808 John Dalton suggested that all matter was made up of tiny spheres that were able to bounce around with perfect elasticity and called them ATOMS
- 3. 2 1898 Joseph John Thompson found that atoms could sometimes eject a far smaller negative particle which he called an ELECTRON
- 4. 1904 Thompson develops the idea that an atom was made up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charge to balance the electron's charge like plums surrounded by pudding. PLUM PUDDING MODEL
- 5. 3 1910 Ernest Rutherford oversaw Geiger and Marsden carrying out his famous experiment. they fired Helium nuclei at a piece of gold foil which was only a few atoms thick. they found that although most of them passed through. About 1 in 10,000 hit
- 6. helium nuclei gold foil helium nuclei They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.
- 7. Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus. He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction However, this was not the end of the story.
- 8. 4 1913 Niels Bohr studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.
- 9. Bohr’s Atom electrons in orbits nucleus
- 11. HELIUM ATOM Shell proton + - N N + electron What do these particles consist of? - neutron
- 12. ATOMIC STRUCTURE Particle Charge Mass proton + ve charge 1 neutron No charge 1 electron -ve charge nil
- 13. ATOMIC STRUCTURE He 2 4 Atomic number the number of protons in an atom Atomic mass the number of protons and neutrons in an atom number of electrons = number of protons
- 14. ATOMIC STRUCTURE Electrons are arranged in Energy Levels or Shells around the nucleus of an atom. • first shell a maximum of 2 electrons • second shell a maximum of 8 electrons • third shell a maximum of 8 electrons
- 15. ATOMIC STRUCTURE There are two ways to represent the atomic structure of an element or compound; 1. 2. Electronic Configuration Dot & Cross Diagrams
- 16. ELECTRONIC CONFIGURATION With electronic configuration elements are represented numerically by the number of electrons in their shells and number of shells. For example; Nitrogen 2 in 1st shell 5 in 2 nd shell configuration = 2 , 5 2 + 5 = 7 N 7 14
- 17. ELECTRONIC CONFIGURATION Write the electronic configuration for the following elements; a) Ca 20 b) Na 40 2,8,8,2 d) Cl 17 35 2,8,7 11 23 c) 2,8,1 e) Si 14 28 2,8,4 O 8 16 2,6 f) B 5 11 2,3
- 18. DOT & CROSS DIAGRAMS With Dot & Cross diagrams elements and compounds are represented by Dots or Crosses to show electrons, and circles to show the shells. For example; X Nitrogen X X N XX X X N 7 14
- 19. DOT & CROSS DIAGRAMS Draw the Dot & Cross diagrams for the following elements; X 8 17 X a) O b) Cl 35 X 16 X X X X X X X X X Cl X X X X X O X X X X X X X X X
- 20. SUMMARY 1. The Atomic Number of an atom = number of protons in the nucleus. 2. The Atomic Mass of an atom = number of Protons + Neutrons in the nucleus. 3. The number of Protons = Number of Electrons. 4. Electrons orbit the nucleus in shells. 5. Each shell can only carry a set number of electrons.
- 21. This powerpoint was kindly donated to www.worldofteaching.com http://www.worldofteaching.com is home to over a thousand powerpoints submitted by teachers. This is a completely free site and requires no registration. Please visit and I hope it will help in your teaching.