Exam 3

Question 1

Degenerate orbitals

Answer 1

Electron orbitals having the same energy levels

Question 1

Aufbau Principle

Answer 1

An electron occupies orbitals in order from lowest energy to highest.

Question 2

Hund’s Rule

Answer 2

Degenerate orbitals are filled evenly before electrons are filled into higher energy levels.

Question 3

Pauli exclusion principle

Answer 3

no more than two electrons can occupy the same orbital and two electrons in the same orbital must have opposite spins

Question 4

Electronegativity

Answer 4

the ability of the atoms to attract electrons from the other elements.

Question 5

Electron affinity

Answer 5

the amount of energy that is released when a molecule acquires an electron

Question 6

Octet rule

Answer 6

the tendency of atoms to prefer to have eight electrons in the valence shell

Question 7

Resonance Structure

Answer 7

a set of two or more Lewis Structures that collectively describe the electronic bonding of a single polyatomic molecule

Question 8

Hybrid Structure

Answer 8

A Lewis structure with multiple ways of being drawn

Question 9

Formal charge

Answer 9

the charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless of relative electronegativity.

Question 9

Expanded octet

Answer 9

occurs when an atom is able to have more than 8 valence electrons

Question 9

Free radical

Answer 9

contain a single unpaired electron in outer orbit

Question 10

bond energy

Answer 10

a measure of the amount of energy needed to break apart one mole of covalently bonded gases

Question 11

Longer bonds

Answer 11

weaker strength

Question 12

VSEPR

Answer 12

a model used to predict 3-D molecular geometry based on the number of valence shell electron bond pairs among the atoms in a molecule or ion

Question 13

how lone pair electrons can distort the bond angles in the molecular geometry

Answer 13

lone pairs occupy more space than bonding pairs and repel the bonding pairs, causing the bond angles to be smaller than expected.

Question 14

Coulomb’s Law

Answer 14

predicts energy of attraction in IMF or chemical bond based on magnitude of charges and distance between particles.

Question 15

dispersion (London) forces

Answer 15

result from fluctuations of electron distribution within neighboring atoms as they move closer together.

Question 16

polar molecules

Answer 16

have permanent dipoles that attract each other through dipole-dipole interactions.

Question 17

Hydrogen Bonding

Answer 17

Special dipole dipole case, Larger change in electronegativity than dipole-dipole, stronger than dipole dipole, between H-N, H-F, and H-O

Question 18

All ionic compounds are

Answer 18

polar - strongest IMFs

Question 19

High Boiling Point =

Answer 19

Strong IMF’s, high molecular weight, high surface area - depends on external pressure

Question 20

Vapor pressure

Answer 20

increases and decreases with temp, but not linear, stays the same no matter the surface area

Question 21

Rate of vaporization

Answer 21

increases with increasing temp and increasing surface area

Question 22

Symmetrical molecules

Answer 22

non-polar

Question 23

An atom in a non-metal compound will have a non-metal partial positive charge if

Answer 23

it is the least electronegative atom

Question 24

Shielding

Answer 24

the core electrons repelling the outer electrons, which lowers the effective charge of the nucleus on the outer electrons.

Question 25

Electron Penetration

Answer 25

An electron gets closer to the nucleus and is held stronger by the Zeff (s is closest, then d, then p)

Question 26

Effective Nuclear charge (Zeff)

Answer 26

the net positive charge pulling electrons towards the nucleus

Question 27

Isoelectronic series

Answer 27

a group of ions that all have the same number of electrons

Question 28

Ionization energy

Answer 28

The energy it takes for an atom to lose an electron

Question 29

dipole moment

Answer 29

a measurement of the separation of two opposite electrical charges

Question 30

1st and 2nd period elements cannot have expanded octets because

Answer 30

do not have access to the the d orbital

Question 31

Anomalous Electron config atoms

Answer 31

Au, Ag, Cu, Mo, Pd, Cr