MCHE 3310 Chapters 1-4 || very Flawless.
Atomic Mass Unit (amu) correct answers 1/12 the mass of a carbon-12 atom
Bohr Model correct answers 1) Electrons revolve around the atomic nucleus in discrete orbitals
2) The position of any particular electron is defined by its orbital
3) The electron energies of electrons are quantized - electrons are permitted to have only specific
values of energy
Wave-Particle Model correct answers 1) Electron exhibits both wave-like and particle-like
characteristics
2) Position of an electron is described by a probability distribution or electron cloud
Quantum Numbers correct answers Set of numbers used to completely describe an electron
Principle Quantum Number correct answers 1) Symbolized by "n"
2) Designates shell
n = 1, 2, 3, 4, 5...
Letter = K, L, M, N, O...
Second Quantum Number correct answers 1) Symbolized by "l"
2) Designates subshell
3) Electron orbital shapes depend upon this
4) Range from 0 to (n - 1)
l = 0, 1, 2, 3...
Subshell = s, p, d, f
Third (Magnetic) Quantum Number correct answers 1) Symbolized by "ml"
2) Determines number of electron orbitals for each subshell
3) It's an integer between -l and +l, including 0
1 s orbital
3 p orbitals
5 d orbitals
7 f orbitals
Fourth Quantum Number correct answers 1) Symbolized by "ms"
2) It's the spin moment and is oriented either up or down (2 electrons per electron orbital)
3) +1/2 for spin up, -1/2 for spin down
Pauli Exclusion Principle correct answers No two electrons in the same atom can have the same
set of four quantum numbers
Orbital Filling Sequence correct answers Electrons tend to occupy the lowest available energy
states.
, Valence Electrons correct answers 1) Most available for bonding and tend to control chemical
properties
2) Present in the outer-most shell
3) For example, When bonding with iron (Fe), even though the 4s subshell has less energy than
the 3d subshell, the iron atom loses the 4s electrons first because they're on the outer-most shell
Electronegativity correct answers 1) Ranges from 0.9 to 4.1
2) Smaller values tend to give away electrons while larger values tend to acquire electrons
Primary Bonding Type: Ionic correct answers 1) Occurs between metallic and nonmetallic
elements
2) Requires electron transfer
3) Large difference in electronegativity required
4) Make for poor conductors and have low chemical reactivity
5) ex. NaCl
Primary Bonding Type: Covalent correct answers 1) Similar Electronegativity (sharing electrons)
2) Bonds are determined by valence, where s & p orbitals dominate bonding
3) Directional bonding between nonmetallic elemental molecules
4) Make for poor conductors and have varying mechanical properties
5) ex. H2
Primary Bonding Type: Metallic correct answers 1) Mainly found in metals and their alloys
2) Valence electrons are not bound to any particular atom and are free to drift through the entire
metal (electrons act as the glue that holds the ion cores together)
3) Non-directional bonding with bonding energy from 62 kJ/mol to 850 kJ/mol
Primary Bonding Combinations correct answers Most materials possess a combination of
different bonds, making generalization of bonding difficult
Secondary Bonding: Van der Waals correct answers 1) Arise from atomic or molecular dipoles
2) Two types of dipoles: induced and permanent
3) Bonding energy around 4-30 kJ/mol
4) Induced dipole ex. H2, Cl2, etc.
5) Permanents dipole ex. HCl, HF, etc.
Secondary Bonding: Hydrogen Bond correct answers 1) Attractive interaction between a
hydrogen atom with an electronegative atom (intermolecular bond)
2) Stronger than Van der Waals interaction but far weaker than covalent or ionic bonds
3) ex. bond between lone pair of oxygen and hydrogen in H2O
Energy and Packing correct answers Dense, ordered packed structures tend to have lower
energies while non-dense, random structures tend to have higher energies
Crystalline Materials correct answers 1) atoms pack in periodic, 3D arrays
2) typical of : metals, many ceramics, some polymers
Atomic Mass Unit (amu) correct answers 1/12 the mass of a carbon-12 atom
Bohr Model correct answers 1) Electrons revolve around the atomic nucleus in discrete orbitals
2) The position of any particular electron is defined by its orbital
3) The electron energies of electrons are quantized - electrons are permitted to have only specific
values of energy
Wave-Particle Model correct answers 1) Electron exhibits both wave-like and particle-like
characteristics
2) Position of an electron is described by a probability distribution or electron cloud
Quantum Numbers correct answers Set of numbers used to completely describe an electron
Principle Quantum Number correct answers 1) Symbolized by "n"
2) Designates shell
n = 1, 2, 3, 4, 5...
Letter = K, L, M, N, O...
Second Quantum Number correct answers 1) Symbolized by "l"
2) Designates subshell
3) Electron orbital shapes depend upon this
4) Range from 0 to (n - 1)
l = 0, 1, 2, 3...
Subshell = s, p, d, f
Third (Magnetic) Quantum Number correct answers 1) Symbolized by "ml"
2) Determines number of electron orbitals for each subshell
3) It's an integer between -l and +l, including 0
1 s orbital
3 p orbitals
5 d orbitals
7 f orbitals
Fourth Quantum Number correct answers 1) Symbolized by "ms"
2) It's the spin moment and is oriented either up or down (2 electrons per electron orbital)
3) +1/2 for spin up, -1/2 for spin down
Pauli Exclusion Principle correct answers No two electrons in the same atom can have the same
set of four quantum numbers
Orbital Filling Sequence correct answers Electrons tend to occupy the lowest available energy
states.
, Valence Electrons correct answers 1) Most available for bonding and tend to control chemical
properties
2) Present in the outer-most shell
3) For example, When bonding with iron (Fe), even though the 4s subshell has less energy than
the 3d subshell, the iron atom loses the 4s electrons first because they're on the outer-most shell
Electronegativity correct answers 1) Ranges from 0.9 to 4.1
2) Smaller values tend to give away electrons while larger values tend to acquire electrons
Primary Bonding Type: Ionic correct answers 1) Occurs between metallic and nonmetallic
elements
2) Requires electron transfer
3) Large difference in electronegativity required
4) Make for poor conductors and have low chemical reactivity
5) ex. NaCl
Primary Bonding Type: Covalent correct answers 1) Similar Electronegativity (sharing electrons)
2) Bonds are determined by valence, where s & p orbitals dominate bonding
3) Directional bonding between nonmetallic elemental molecules
4) Make for poor conductors and have varying mechanical properties
5) ex. H2
Primary Bonding Type: Metallic correct answers 1) Mainly found in metals and their alloys
2) Valence electrons are not bound to any particular atom and are free to drift through the entire
metal (electrons act as the glue that holds the ion cores together)
3) Non-directional bonding with bonding energy from 62 kJ/mol to 850 kJ/mol
Primary Bonding Combinations correct answers Most materials possess a combination of
different bonds, making generalization of bonding difficult
Secondary Bonding: Van der Waals correct answers 1) Arise from atomic or molecular dipoles
2) Two types of dipoles: induced and permanent
3) Bonding energy around 4-30 kJ/mol
4) Induced dipole ex. H2, Cl2, etc.
5) Permanents dipole ex. HCl, HF, etc.
Secondary Bonding: Hydrogen Bond correct answers 1) Attractive interaction between a
hydrogen atom with an electronegative atom (intermolecular bond)
2) Stronger than Van der Waals interaction but far weaker than covalent or ionic bonds
3) ex. bond between lone pair of oxygen and hydrogen in H2O
Energy and Packing correct answers Dense, ordered packed structures tend to have lower
energies while non-dense, random structures tend to have higher energies
Crystalline Materials correct answers 1) atoms pack in periodic, 3D arrays
2) typical of : metals, many ceramics, some polymers
