Development of the Modern Atomic Theory
... 1. All matter is composed of atoms, which are tiny, indivisible particles. 2. A chemical reaction is a rearrangement of atoms to form different compounds. Atoms are neither created nor destroyed in a chemical reaction (the law of conservation of mass). 3. Atoms of one element cannot be converted int ...
... 1. All matter is composed of atoms, which are tiny, indivisible particles. 2. A chemical reaction is a rearrangement of atoms to form different compounds. Atoms are neither created nor destroyed in a chemical reaction (the law of conservation of mass). 3. Atoms of one element cannot be converted int ...
Population Analysis
... This result suggests that we take, 2Ca2 as a measure of the number of electrons "on" or "associated" with center a and 4CaCb ∆ ab as a measure of the number of electrons in the region between and common to both nuclei. This interpretation was put forth by R. Mulliken (J. Chem Phys 1955, 23, 1833) a ...
... This result suggests that we take, 2Ca2 as a measure of the number of electrons "on" or "associated" with center a and 4CaCb ∆ ab as a measure of the number of electrons in the region between and common to both nuclei. This interpretation was put forth by R. Mulliken (J. Chem Phys 1955, 23, 1833) a ...
Key vocabulary of the week
... Term: wave Definition: an amount of energy (such as light) traveling through space-time in an up and down shape (resembling a wave) ...
... Term: wave Definition: an amount of energy (such as light) traveling through space-time in an up and down shape (resembling a wave) ...
Atomic Mass Review Sheet
... element. Remember it this way, atomic weight is a weighted average. Units: none Molecular Mass The molecular mass is the mass of a molecule. It is calculated by adding together the atomic masses in the molecule. Units: amu Molar Mass The molar mass is the mass of an element or molecule present in 1 ...
... element. Remember it this way, atomic weight is a weighted average. Units: none Molecular Mass The molecular mass is the mass of a molecule. It is calculated by adding together the atomic masses in the molecule. Units: amu Molar Mass The molar mass is the mass of an element or molecule present in 1 ...
Glossary - WordPress.com
... When gas molecule collides with each other their total energy does not decrease or increase. This type of collision is called an elastic collision. ...
... When gas molecule collides with each other their total energy does not decrease or increase. This type of collision is called an elastic collision. ...
CHAPTER TWO ATOMS, MOLECULES, AND IONS
... a. Dinitrogen monoxide is correct. N and O are both nonmetals resulting in a covalent compound. We need to use the covalent rules of nomenclature. The other two names are for ionic compounds. b. Copper(I) oxide is correct. With a metal in a compound, we have an ionic compound. Because copper, like m ...
... a. Dinitrogen monoxide is correct. N and O are both nonmetals resulting in a covalent compound. We need to use the covalent rules of nomenclature. The other two names are for ionic compounds. b. Copper(I) oxide is correct. With a metal in a compound, we have an ionic compound. Because copper, like m ...
CHAPTER TWO ATOMS, MOLECULES, AND IONS For Review 1. a
... a. Dinitrogen monoxide is correct. N and O are both nonmetals resulting in a covalent compound. We need to use the covalent rules of nomenclature. The other two names are for ionic compounds. b. Copper(I) oxide is correct. With a metal in a compound, we have an ionic compound. Because copper, like m ...
... a. Dinitrogen monoxide is correct. N and O are both nonmetals resulting in a covalent compound. We need to use the covalent rules of nomenclature. The other two names are for ionic compounds. b. Copper(I) oxide is correct. With a metal in a compound, we have an ionic compound. Because copper, like m ...
1 The modern model of the atom is based on the work of (1) one
... provided below, show a correct numerical setup for calculating the average atomic mass of neon. [1] ...
... provided below, show a correct numerical setup for calculating the average atomic mass of neon. [1] ...
isuintroduction
... mole) as a base to compare with all other elements on the periodic table.(2) 1 mole of Carbon-12 weighed 24 grams. Therefore, 24 grams of Carbon in ratio to 2 grams of hydrogen, after reducing to simplest form and relative atomic weight, would equal 12 grams of Carbon in ratio to 1 gram of hydrogen. ...
... mole) as a base to compare with all other elements on the periodic table.(2) 1 mole of Carbon-12 weighed 24 grams. Therefore, 24 grams of Carbon in ratio to 2 grams of hydrogen, after reducing to simplest form and relative atomic weight, would equal 12 grams of Carbon in ratio to 1 gram of hydrogen. ...
chemistry 101 spring 2002 part 1
... Directions: (1) Put your name, S.I.D. number and signature on the free response part of the exam where indicated. (2) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decid ...
... Directions: (1) Put your name, S.I.D. number and signature on the free response part of the exam where indicated. (2) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decid ...
As part of our Chemistry unit, you will create and share a model of
... distinguish between each of the subatomic particles (they will each look different). Please make sure that they are secure on your model and will not fall off. It is your responsibility to make sure that everything stays in place until I am able to grade it. You must also identify the element and te ...
... distinguish between each of the subatomic particles (they will each look different). Please make sure that they are secure on your model and will not fall off. It is your responsibility to make sure that everything stays in place until I am able to grade it. You must also identify the element and te ...
class 2.pptx
... Chlorine is a mixture of two isotopes : 35Cl, 75.8%, and 37Cl, 24.2%. Chlorine occurs as Cl2 molecules. A mass spectrometer can be used to measure the mass of molecules - not bulk samples. In this case, this is done by making Cl2+ ions and using their charge-to-mass ratios to distinguish the masses ...
... Chlorine is a mixture of two isotopes : 35Cl, 75.8%, and 37Cl, 24.2%. Chlorine occurs as Cl2 molecules. A mass spectrometer can be used to measure the mass of molecules - not bulk samples. In this case, this is done by making Cl2+ ions and using their charge-to-mass ratios to distinguish the masses ...
class 2.pptx
... t A mass spectrometer can be used to measure the mass of molecules - not bulk samples. In this case, this is done by making Cl2+ ions and using their charge-to-mass ratios to distinguish the masses of isotopically different Cl2+ ions (like Thomson’s expt.) . t How many different masses can Cl2+ io ...
... t A mass spectrometer can be used to measure the mass of molecules - not bulk samples. In this case, this is done by making Cl2+ ions and using their charge-to-mass ratios to distinguish the masses of isotopically different Cl2+ ions (like Thomson’s expt.) . t How many different masses can Cl2+ io ...
Laboratory Pb Name: Date: ______ (1) Measure the mass of a
... (5) Table S in the Chemistry Reference Tables lists the accepted value for the density of lead. Calculate your percent error. Show all work. ...
... (5) Table S in the Chemistry Reference Tables lists the accepted value for the density of lead. Calculate your percent error. Show all work. ...
Honors Review for Semester 1 Final 2014
... 1. The story of the Atom: know the major atomic scientists and their contributions towards atomic theory: Democritus (ancient Greeks), Dalton, Thomson, Rutherford 2. You should also be able to illustrate the above scientists’ models of the atoms, labeling subatomic particles. 3. Define atom, nucleus ...
... 1. The story of the Atom: know the major atomic scientists and their contributions towards atomic theory: Democritus (ancient Greeks), Dalton, Thomson, Rutherford 2. You should also be able to illustrate the above scientists’ models of the atoms, labeling subatomic particles. 3. Define atom, nucleus ...
Chapter 2
... both are carbon, must have 6 protons 12C has 6 protons and 6 neutrons 14C has 6 protons and 8 neutrons ...
... both are carbon, must have 6 protons 12C has 6 protons and 6 neutrons 14C has 6 protons and 8 neutrons ...
Chapter 2 - Atoms, Molecules, and Ions
... I. It is sometimes equal to the empirical formula. II. It is always a whole number multiple of the empirical formula III. It indicates the exact number and the identities of the atoms that make up a molecule. A. I only B. II only C. I and II only D. I, II, and III A 92-2. How many atoms are in 12 mo ...
... I. It is sometimes equal to the empirical formula. II. It is always a whole number multiple of the empirical formula III. It indicates the exact number and the identities of the atoms that make up a molecule. A. I only B. II only C. I and II only D. I, II, and III A 92-2. How many atoms are in 12 mo ...
Chemistry Unit Notes Organizing the Periodic Table All the elements
... 1. State what happens to the distance between particles when a substance changes a. from a solid to a gas b. from a liquid to a solid 2. Why is it easier to compress a gas than a liquid? 3. What causes a solid to have a definite shape and volume? 4. Gas particles are considered to have very little a ...
... 1. State what happens to the distance between particles when a substance changes a. from a solid to a gas b. from a liquid to a solid 2. Why is it easier to compress a gas than a liquid? 3. What causes a solid to have a definite shape and volume? 4. Gas particles are considered to have very little a ...
Atoms, Molecules and Ions
... abundance of 7.5% and an atomic mass of 6.015122 amu. Lithium-7 has a natural abundance of 92.5% and an atomic mass of 7.016003 amu. ...
... abundance of 7.5% and an atomic mass of 6.015122 amu. Lithium-7 has a natural abundance of 92.5% and an atomic mass of 7.016003 amu. ...
FALL Final Review KEY
... 35. Ionic: transfer of electrons between one metal and one nonmetal Covalent: sharing of electrons between two nonmetals (including hydrogen) Metallic: electron sea model (fixed positive cations and delocalized negative valence electrons) a. Covalent b. Covalent electrons shared and Ionic bonds ...
... 35. Ionic: transfer of electrons between one metal and one nonmetal Covalent: sharing of electrons between two nonmetals (including hydrogen) Metallic: electron sea model (fixed positive cations and delocalized negative valence electrons) a. Covalent b. Covalent electrons shared and Ionic bonds ...
AS Unit F321 Unit 1 Side A check list
... mass. Describe the distribution of mass and charge within an atom. Describe the contribution of protons and neutrons to the nucleus of an atom, in terms of atomic (proton) number and mass (nucleon) number. Deduce the numbers of protons, neutrons and electrons in: (i) ...
... mass. Describe the distribution of mass and charge within an atom. Describe the contribution of protons and neutrons to the nucleus of an atom, in terms of atomic (proton) number and mass (nucleon) number. Deduce the numbers of protons, neutrons and electrons in: (i) ...
Document
... you to a birthday party! 50 years ago, Illinois alumnus Nick Holonyak Jr. demonstrated the first visible light-emitting diode (LED) while working at GE. Holonyak returned to Illinois as a professor in 1963, and has been unveiling new inventions on our campus ever since. Today, the LED he demonstrate ...
... you to a birthday party! 50 years ago, Illinois alumnus Nick Holonyak Jr. demonstrated the first visible light-emitting diode (LED) while working at GE. Holonyak returned to Illinois as a professor in 1963, and has been unveiling new inventions on our campus ever since. Today, the LED he demonstrate ...
Chemical Context of Life
... isotopes = atoms of an element with the same atomic number but different atomic masses • have the same #protons but a different number of neutrons • physical properties differ, but chemical properties remain unchanged ...
... isotopes = atoms of an element with the same atomic number but different atomic masses • have the same #protons but a different number of neutrons • physical properties differ, but chemical properties remain unchanged ...
BIOCHEMISTRY: The Chemistry of Life Chemistry of Life: ATOMS
... • Atoms have an EQUAL number of protons and electrons • Ions have an UNEQUAL number of protons and electrons, have a CHARGE – Cation: more protons than electrons, POSITIVE charge, LOSE electrons – Anion: more electrons than protons, NEGATIVE charge, GAIN electrons ...
... • Atoms have an EQUAL number of protons and electrons • Ions have an UNEQUAL number of protons and electrons, have a CHARGE – Cation: more protons than electrons, POSITIVE charge, LOSE electrons – Anion: more electrons than protons, NEGATIVE charge, GAIN electrons ...
Proton
The proton is an elementary subatomic particle, symbol p or p+, with a positive electric charge of +1e elementary charge and mass slightly less than that of a neutron. Protons and neutrons, each with mass approximately one atomic mass unit, are collectively referred to as ""nucleons"". One or more protons are present in the nucleus of an atom. The number of protons in the nucleus is referred to as its atomic number. Since each element has a unique number of protons, each element has its own unique atomic number. The word proton is Greek for ""first"", and this name was given to the hydrogen nucleus by Ernest Rutherford in 1920. In previous years Rutherford had discovered that the hydrogen nucleus (known to be the lightest nucleus) could be extracted from the nuclei of nitrogen by collision. The proton was therefore a candidate to be a fundamental particle and a building block of nitrogen and all other heavier atomic nuclei.In the modern Standard Model of particle physics, the proton is a hadron, and like the neutron, the other nucleon (particle present in atomic nuclei), is composed of three quarks. Although the proton was originally considered a fundamental particle, it is composed of three valence quarks: two up quarks and one down quark. The rest masses of the quarks contribute only about 1% of the proton's mass, however. The remainder of the proton mass is due to the kinetic energy of the quarks and to the energy of the gluon fields that bind the quarks together. Because the proton is not a fundamental particle, it possesses a physical size; the radius of the proton is about 0.84–0.87 fm.At sufficiently low temperatures, free protons will bind to electrons. However, the character of such bound protons does not change, and they remain protons. A fast proton moving through matter will slow by interactions with electrons and nuclei, until it is captured by the electron cloud of an atom. The result is a protonated atom, which is a chemical compound of hydrogen. In vacuum, when free electrons are present, a sufficiently slow proton may pick up a single free electron, becoming a neutral hydrogen atom, which is chemically a free radical. Such ""free hydrogen atoms"" tend to react chemically with many other types of atoms at sufficiently low energies. When free hydrogen atoms react with each other, they form neutral hydrogen molecules (H2), which are the most common molecular component of molecular clouds in interstellar space. Such molecules of hydrogen on Earth may then serve (among many other uses) as a convenient source of protons for accelerators (as used in proton therapy) and other hadron particle physics experiments that require protons to accelerate, with the most powerful and noted example being the Large Hadron Collider.