general chem

Question 1

effective nuclear charge _______ from left to right in periods

Answer 1

increases

Question 2

as you move down elements of given group, ____ increases by one each time

Answer 2

principle quantum number

Question 3

Zeff is _____ in groups

Answer 3

pretty consistent

Question 4

atomic radius refers to ______, while ionic radius is dependent on ________

Answer 4

size of neutral element

how the element ionizes based on its element type and group #

Question 5

______ is essentially the opposite that of all other periodic trends

Answer 5

atomic radius

Question 6

while other periodic trends _________ going up and to the right, atomic radius _______ going down and to the right

Answer 6

increase
increase

Question 7

metals ______ e- and become ______

Answer 7

lose
positive

Question 8

non metals ______ e- and become ____

Answer 8

gain
negative

Question 9

the nonmetals close to the metalloid line possess a ___ ionic radius than their counterparts closer to group VIIIA

Answer 9

larger

Question 10

metals closer to the metalloid line have ______ e- to lose to achieve the electronic configuration seen in group VIIIA

Answer 10

more

Question 11

noble gases are known as ____ because they have minimal chemical reactivity due to their filled valence shells

Answer 11

inert gases

Question 12

the ng have _ boiling points

Answer 12

low

Question 13

transition elements are considered to be ___ and have _ electron affinitites, ionization energies, and electronegativities

Answer 13

metals
low

Question 14

transition metals are capable of losing what

Answer 14

different numbers of e- from s and d orbitals in their valence shells

Question 15

_______ only need one more electron to have a noble gas-like configuration

Answer 15

halogens

Question 16

chalcogens

Answer 16

group of non metals and mealloids
size e- in their valence electron shell
small atomic radii and large ionic radii

oxygen is most important element in this group
selenium important for microorganims
at high conc many of these elements can be toxic or damaging

Question 17

alkaline earth metals

Answer 17

slightly higher effective nuclear charges and slighl smaller atomic radii than alkali metals

two e- in valence shell

alkali and alkaline earth metals togt called active metals

Question 18

alkali metals

Answer 18

densities lower than other metals

one loosely bound e- in outermost shells
Zeff values low
largest atomic radii of all elemetns in respective periods
low ionization nrg
low e- affinity low electronegativity

Question 19

pauling electronegativity scale

Answer 19

0.7 cesium

4.0 flourine

Question 20

electronegativity ____ across period from l to r and __ in group from t to b

Answer 20

increases
decreases

Question 21

e- affinity is what

Answer 21

energy dissipated by gaseous species when it gains and e-

Question 22

electron affinity ____ across period from l to r and what from t to b

Answer 22

increases
decreases

Question 23

noble gases have what electron affiniteis

Answer 23

zero

Question 24

ionization energy is what

Answer 24

energy required to remove an e- from gaseous species

Question 25

electron affinity is a what process

Answer 25

exothermic

Question 26

ionization energy is a what process

Answer 26

endothermic

Question 27

ionzation energy trend

Answer 27

increases from l to r decreases t to b

Question 28

first ionization energy will be ____ than second, will be_____ than third, etc...

Answer 28

smaller smaller

Question 29

what are the exceptions to the octet rule?

Answer 29

incomplete octet: stable with fewer than 8 electrons in their valence shell and include hydrogen 2, helium 2,lithium 2, beryllium 4, and boron 6 expanded octet: any element in period 3 and greater can hold more than 8 electrons, phosphorus 10 sulfur 12, chlorin 15, and many others odd number of electrons: any molecule with odd number of valence electrons cannot distribute those electrons to give eight to each atom - nitric oxide 11

Question 30

ionic bonding

Answer 30

one or more electrons from an atom with a low ionization energy - typically a metal, are transferred to an atom with high electron affinity - typically nonmetal

Question 31

covalent bonding

Answer 31

electron pair is shared between two atoms - typically nonmetals that have relatively similar values of EN

Question 32

coordinate covalent

Answer 32

if both shared electrons are contributed by only one of the two atoms generally means lone pair of one atom attacked another atom with an unhybridized p orbital to form a bond

Question 33

ionic compounds melting boiling point etc

Answer 33

high melting / boiling point

Question 34

bond length

Answer 34

avg distance between two nuclei of atoms in a bond

Question 35

bond energy

Answer 35

energy required to break a bond by separating its components into their isolated gaseous atomic states

Question 36

electronic geometry

Answer 36

spatial arragenment of all pairs of electrons around the central atom, including both the bonding and lone pairs

Question 37

molecular eometry

Answer 37

describes spatial arrangement of only the bonding pairs of electronsco

Question 38

coordination number

Answer 38

number of atoms that surround and are bonded to a central atom

Question 39

when orbitals overlap head to head, the resulting bond is a what bond

Answer 39

sigma they allow for free roation about their axes because the electron density of the bonding orbital is a single linear acumulation between atomic nuclei

Question 40

when orbitals overlap in such a way that there are two parallel electron cloud densities, a what bond is formed?

Answer 40

pi do not allow for free rotation because the electron densities of the orbitals are parllel and cannot be twisted in such a way that allows continous overlapping of the clouds of electron densities

Question 41

law of constant composition

Answer 41

any pure sample of given compound will contain same elements in an identical mass ratio

Question 42

types of rxns

Answer 42

combination rxn decomposition rxn combustion single displacement double displacement neutralization

Question 43

_____ compounds make good electrolytes becaue they dissolve the most readily

Answer 43

ionic

Question 44

_____ compounds are the weakest because they do not form current-carrying ions

Answer 44

nonpolar covalent compounds

Question 45

collision theory of chemcial kinetics

Answer 45

the rate of a reaction is proportional to the number of collisions per second between the reaacting molecules

Question 46

low activation energy and high temp make the negative exponnent of arrhenius equation ____ in magnitude and thus ____ the rate constant, k

Answer 46

smaller increases

Question 47

factors affecting rxn rate

Answer 47

reactant conntrations temp medium catalysts

Question 48

the greater the conc of the reactants, the ____ the number of effective collisions per unit time

Answer 48

greater rxn rate will increase for all but zero order rxns

Question 49

homogenous and heterogenous catalysis

Answer 49

catalyst is in same phase as reactants caalye is in distinct phase

Question 50

what are the only things that can change the rate of a zero order reaction?

Answer 50

temperature and addition of catalyst

Question 51

isothermal processes adiabatic processes isobaric isovlumetric / isochoric

Answer 51

systems temp is constant no heat is exchaged between syste and enviornment pressure is contstant no change in volume

Question 52

hess' law states what

Answer 52

enthalpy changes of reactions are additive

Question 53

boyles law

Answer 53

pressure and volume inversely related

Question 54

charles' law

Answer 54

volume and temperature are directly proportional

Question 55

the ______ of a gas will increase with increasing partial pressu reo fthe gas

Answer 55

solubility

Question 56

chelation

Answer 56

central cation can be bonded to the same ligand in multiple places

Question 57

_______ and ______ cells house spontaneous reactions, while _____ cells contain nonspontaneous reactions

Answer 57

galvanic concentration electrolytic

Question 58

purpose of salt bridge

Answer 58

exchange anions and cations to balance, or dissipate newly generated charges

Question 59

energy density in batteries

Answer 59

measure of a battery's ability to produce power as a function of its weight

Question 60

isoelectric focusing

Answer 60

separate amino acids or polypeptides basedo n their isoelectric points