Review Outline for Atomic Structure Test
... A) Subatomic particles a. What are the atomic mass units for protons, neutrons, and electrons? Protons and neutrons = 1 amu; electrons about 0 amu What does the atomic number represent? # of protons b. What does the mass number represent? # of protons + # of neutrons c. What particles are in equal n ...
... A) Subatomic particles a. What are the atomic mass units for protons, neutrons, and electrons? Protons and neutrons = 1 amu; electrons about 0 amu What does the atomic number represent? # of protons b. What does the mass number represent? # of protons + # of neutrons c. What particles are in equal n ...
File
... the mass of the products equals 80g (Law of conservation of mass). You should also notice that in CH4 there is one Carbon atom, and four hydrogen atoms (Law of definite proportions). Electrolysis Reactions: Carried out in a Hoffman’s apparatus (shown to the right), it splits water compounds into o ...
... the mass of the products equals 80g (Law of conservation of mass). You should also notice that in CH4 there is one Carbon atom, and four hydrogen atoms (Law of definite proportions). Electrolysis Reactions: Carried out in a Hoffman’s apparatus (shown to the right), it splits water compounds into o ...
An element`s properties depend on the structure of its atoms
... • A ball bouncing down a flight of stairs provides an analogy for energy levels of electrons, because the ball can come to rest only on each step, not between steps. • It’s a quantized event! ...
... • A ball bouncing down a flight of stairs provides an analogy for energy levels of electrons, because the ball can come to rest only on each step, not between steps. • It’s a quantized event! ...
form revision a
... Check your key area statements. If not green you need to do more work! Knowledge of the structure of the periodic table, groups and periods. All matter is made of atoms. When a substance contains only one kind of atom it is known as an element. Atoms contain protons, neutrons and electrons each with ...
... Check your key area statements. If not green you need to do more work! Knowledge of the structure of the periodic table, groups and periods. All matter is made of atoms. When a substance contains only one kind of atom it is known as an element. Atoms contain protons, neutrons and electrons each with ...
Atoms and the Particles They Contain Chemistry Packet: Honors
... Neutrons are also found in the nucleus of an atom. Neutrons are neutral with no charge and have a mass of 1 amu, just like the proton. Electrons are found constantly moving around the nucleus in a random fashion. For teaching purposes we say that electrons travel in electron clouds or energy levels ...
... Neutrons are also found in the nucleus of an atom. Neutrons are neutral with no charge and have a mass of 1 amu, just like the proton. Electrons are found constantly moving around the nucleus in a random fashion. For teaching purposes we say that electrons travel in electron clouds or energy levels ...
Chapter 9: Chemical Bonding I: Lewis Theory
... A) Ionic Bonding results from electron transfer. B) Occurs between metals & nonmetals. i) Metals lose electrons to form cations while nonmetals gain electrons to form anions. C) Ion pair is more stable than separated ions. D) Found as a 3-D crystal lattices containing alternating cations & anions. 2 ...
... A) Ionic Bonding results from electron transfer. B) Occurs between metals & nonmetals. i) Metals lose electrons to form cations while nonmetals gain electrons to form anions. C) Ion pair is more stable than separated ions. D) Found as a 3-D crystal lattices containing alternating cations & anions. 2 ...
Quantum Coherence between States with Even and Odd Numbers of Electrons
... introduced the superselection rule, according to which such linear superpositions are physically impossible. In actuality (as was pointed out in [2, 3]), the superselection rule is the alternative to the existence, along with x, y, z, and t, of additional spinor coordinates, which, in fact, are intr ...
... introduced the superselection rule, according to which such linear superpositions are physically impossible. In actuality (as was pointed out in [2, 3]), the superselection rule is the alternative to the existence, along with x, y, z, and t, of additional spinor coordinates, which, in fact, are intr ...
Chem1101 – Semester 1
... Heteronuclear molecules: are formed through the mixing of different atomic orbitals gives rise to asymmetric molecular orbitals The bond between two elements with different electronegativities will be polar. Th ...
... Heteronuclear molecules: are formed through the mixing of different atomic orbitals gives rise to asymmetric molecular orbitals The bond between two elements with different electronegativities will be polar. Th ...
Worksheet 20.2
... 1- Atoms can achieve a noble gas structure by gaining, losing or sharing electrons with other atoms. 2- The rule states that, except for hydrogen , an atom combines with other atoms to form bonds in order to have 8 electrons in its valence energy level ( like noble gases). Lewis dot symbols are repr ...
... 1- Atoms can achieve a noble gas structure by gaining, losing or sharing electrons with other atoms. 2- The rule states that, except for hydrogen , an atom combines with other atoms to form bonds in order to have 8 electrons in its valence energy level ( like noble gases). Lewis dot symbols are repr ...
Chem 115 POGIL Worksheet - Week 10 Periodic Trends Why? The
... Ionization energy, I, is the energy required to remove an electron from a gaseous species. The first ionization energy, I1, refers to removing one electron from a neutral atom: X(g) X+(g) + e– ...
... Ionization energy, I, is the energy required to remove an electron from a gaseous species. The first ionization energy, I1, refers to removing one electron from a neutral atom: X(g) X+(g) + e– ...
PPT
... No two electrons can be in the same quantum state. For example, in a given atom they cannot have the same set of quantum numbers n, l, ml, ms. This means that each atomic orbital (n,l,ml) can hold 2 electrons: ms = ±½. Important consequence: Electrons do not pile up in the lowest energy state. It’ ...
... No two electrons can be in the same quantum state. For example, in a given atom they cannot have the same set of quantum numbers n, l, ml, ms. This means that each atomic orbital (n,l,ml) can hold 2 electrons: ms = ±½. Important consequence: Electrons do not pile up in the lowest energy state. It’ ...
Chapter 2
... ion - any atom with a positive or negative charge anion - atom with a NEGATIVE charge cation - atom with a POSITIVE charge ...
... ion - any atom with a positive or negative charge anion - atom with a NEGATIVE charge cation - atom with a POSITIVE charge ...
Adv review key
... A) Electrons are transferred between atoms B) Valence electrons- outer shell electrons C) Metals a. Lend valence electrons b. 1 – 4 valence electrons c. Form positive ions ( more protons than electrons) D) Nonmetals a. Borrow valence electrons b. 4 - 8 valence electrons c. Form negative ions (more e ...
... A) Electrons are transferred between atoms B) Valence electrons- outer shell electrons C) Metals a. Lend valence electrons b. 1 – 4 valence electrons c. Form positive ions ( more protons than electrons) D) Nonmetals a. Borrow valence electrons b. 4 - 8 valence electrons c. Form negative ions (more e ...
APS 1st semester exam review 2016
... A) Electrons are transferred between atoms B) Valence electrons- outer shell electrons C) Metals a. Lend valence electrons b. 1 – 4 valence electrons c. Form positive ions ( more protons than electrons) D) Nonmetals a. Borrow valence electrons b. 4 - 8 valence electrons c. Form negative ions (more e ...
... A) Electrons are transferred between atoms B) Valence electrons- outer shell electrons C) Metals a. Lend valence electrons b. 1 – 4 valence electrons c. Form positive ions ( more protons than electrons) D) Nonmetals a. Borrow valence electrons b. 4 - 8 valence electrons c. Form negative ions (more e ...
Bohr model
In atomic physics, the Rutherford–Bohr model or Bohr model, introduced by Niels Bohr in 1913, depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity. After the cubic model (1902), the plum-pudding model (1904), the Saturnian model (1904), and the Rutherford model (1911) came the Rutherford–Bohr model or just Bohr model for short (1913). The improvement to the Rutherford model is mostly a quantum physical interpretation of it. The Bohr model has been superseded, but the quantum theory remains sound.The model's key success lay in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen. While the Rydberg formula had been known experimentally, it did not gain a theoretical underpinning until the Bohr model was introduced. Not only did the Bohr model explain the reason for the structure of the Rydberg formula, it also provided a justification for its empirical results in terms of fundamental physical constants.The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems (see below for application), the Bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atom. A related model was originally proposed by Arthur Erich Haas in 1910, but was rejected. The quantum theory of the period between Planck's discovery of the quantum (1900) and the advent of a full-blown quantum mechanics (1925) is often referred to as the old quantum theory.