Book Notes

Question 1

proton charge

Answer 1

e = 1.6e-19 C

Question 2

atomic #

Answer 2

Z = proton #

Question 3

Mass #

Answer 3

A = proton + neutron

Question 4

electrons charge

Answer 4

e = - 1.6e-19 C

Question 5

protium

Answer 5

1 amu (1 proton)

Question 6

tritium

Answer 6

3 amu (1 proton, 2 neutrons)

Question 7

Planck relation

Answer 7

E = hf

Question 8

Planck constant

Answer 8

6.626e-34 J•s

Question 9

Bohr model

Answer 9

L = (nh)/(2π)

Question 10

Angular momentum

Answer 10

L = mvr

Question 11

Rydberg equation

Answer 11

E = RH/n²

Question 12

Rydberg constant

Answer 12

2.18e-18 J/electron

Question 13

the energy of an electron (increases/decreases) becomes (more/less) negative the farther out from the nucleus that it is located in

Answer 13

the energy of an electron increses becomes less negative the farther out from the nucleus that it is located in

Question 14

Pauli exclusion principle

Answer 14

no two electrons can have he same set of 4 quantum #s

Question 15

Lyman series

Answer 15

n≥2 to n=1

Question 16

Balmer series

Answer 16

n ≥ 3 to n = 2

Question 17

Paschen series

Answer 17

n ≥ 4 to n = 3

Question 18

Max # of electrons w/in a shell

Answer 18

2n

Question 19

Aufbau principle

Answer 19

order in which subshells are filled (N + 1 rule) ranks subshells in increasing energy

Question 20

Hund’s rule

Answer 20

orbitals are filled so that there are a max # of ahlf-filled orbitals w/ parallel spins

Question 21

exceptions to hunds rule

Answer 21

chromium (z = 24) and its groups

copper and its grou

F -subshells

Question 22

Paramagnetic

Answer 22

atoms w/ unpaired electrons

Question 23

diamagnetic

Answer 23

paired electrons

Question 24

Effective nuclear charge (Z_eff)

Answer 24

electrostatic atraction b/t valence shell electrons and the nucleus; a measure of the net positive charge experienced by the outermost electrons

Question 25

Periodic trends for electronegativiity, ionization energy, atomic radius, and electron affinity

Answer 25

electronegativity, ionization energy, and electron affinity increase up and right; atomic radius increases up and down

Question 26

Ionic bonding

Answer 26

electrons form.an atom w/ a low ionization energy are transferred to an atom with high electron affinity (typically occurs between metal and nonmetal)

Question 27

Covalent bonding

Answer 27

an electron pair is shared b/t two atoms (typically nonmetals)

Question 28

Coordinate covalent bonding

Answer 28

If both of the shared electrons are contributed by only 1 of the 2 atoms

Question 29

Polar covalent vs. nonpolar covalent

Answer 29

Nonpolar covalent bonds are a type of chemical bond where two atoms share a pair of electrons with each other. Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms

Question 30

Bond order

Answer 30

the # of shared electron pairs b/t 2 atoms

Question 31

Bond length trend

Answer 31

As # of shared electron pairs increase, bond length decreases

Question 32

bond energy definition and trend

Answer 32

it is the amount of energy required to break a bond; greater # of pairs of electrons shared b/t the atomic nuclei;

Question 33

bond length relationship with bond energy

Answer 33

single bond = longest and weakest

triple bond = shortest and strongest

Question 34

how to calculate the dipole moment

Answer 34

Dipole moment p = qd

dipole moment = the magnitude of the charge * the displacement vector separating the two partial charges

Question 35

Formal charge definition and calculation

Answer 35

formal charge: difference b/t the # of electrons asisgned to an atom in a Lewis structure and teh # of electrons normally found int he atom’s valence shell

Formal charge = V-Nonbonding - (1/2)Nonbonding

Question 36

Electronic geometry vs. molecular geometry

Answer 36

Electronic geometry = spatial arrangement of all pairs of electrons (both bonding and nonbonding) and determines the ideal bond angle while the molecular geometry includes only the bonding pairs