Gen chem 2

Question 1

rows of the periodic table are called?

Answer 1

periods

Question 2

columns of the PT are called ?

Answer 2

groups or families

Question 3

electrons located where have the highest potential energy?

Answer 3

they are located in the valence shell

Question 4

Offhand, what are the electron configurations for chromium and copper`

Answer 4

for chromium its 4s^1 3d^5

for copper its 4s^1 3d^10

Question 5

what element is a metal but not considered lustrous and why?

Answer 5

mercury, because its a liquid under standard conditions

Question 6

name ten qualities of metals, starting with high melting point?
Also what quality about metals do many of these characteristics point to?

Answer 6

high melting point, high densities, malleable, ductile,

Low effective nuclear charge, low electronegativity(high electropositivity), large atomic radius, small ionic radius, low ionization energy, low electron affinity(these qualities point to how metals lose electrons easily

Question 7

what quality about the valence e-‘s of metals makes them good conductors of heat and electricity

Answer 7

its because their valence electrons are loosely bound to atoms

Question 8

where are the valence electrons of active metals, transition metals, actinides and lanthanides

Answer 8

s subshell; s and d subshells, s and f subshells

Question 9

name 9 qualities of nonmetals

Answer 9

brittle
high ionization energy
high electron affinity
high electronegativity(low electropositivity)
small atomic radius
large ionic radius
poor conductors of heat
poor conductor of electricity
doesn't give up electrons easily

Question 10

name the metalloids

Answer 10

boron, silicon, germanium, arsenic, antimony, tellurium, polonium, and astatine

Question 11

how does the positivity of the nucleus increase? and with this what force increases?what charge is known as?

Answer 11

it increases from left to right, because protons increase with atomic number!
also, because this positivity is increasing, the electrostatic attraction between the valence electron shell electrons and the nucleus will increase(this is called the effective nuclear charge)

Question 12

what is the zeff a measure of? how does zeff increase on the PT?

Answer 12

the zeff is a measure of the net positive charge experienced by the outermost electrons—this pull is done by the inner electrons
-zeff increases from left to right within a period

Question 13

why are valence electrons held less tightly as you move down a group

Answer 13

this is due to the increased separation between the valence electrons and the nucleus

Question 14

what is the atomic radius?

how it increase?

Answer 14

atomic radius of an element is equal to one-half of the distance btween the centers of the two atoms of an element that are briefly in contact with each other
atomic radius increases from right to left

Question 15

what does ionic radius depend on?

Answer 15

it depends on how the element ionizes based on its element type and group number

Question 16

what does the group number of nonmetals close to the metalloid line tell us?

Answer 16

their group number tells us that they need more electrons than other nonmetals to get to an electronic configuration like the ones the inert gases have

Question 17

how do metals close to the metalloid line achieve an inert gas like electronic configuration

Answer 17

they need to lose electrons for this to happen

Question 18

why do metals close to the metalloid line have a greater ionic radius than inert gases?

Answer 18

they do because they lose electrons

Question 19

what is ionization energy

Answer 19

it is the energy required to remove an electron from a gas species

Question 20

is removing an electron from an atom exo or endothermic

Answer 20

endo, it always requires energy

Question 21

what is a reason that valence electrons are tightly bound to an atom
how does this affect the ionization energy

Answer 21

atom has a high zeff, which means that the atom’s valence electrons are close to the nucleus
this makes it difficult to remove electrons and increases their ionization energy

Question 22

how does ionization energy increase in a period and a group in the PT

Answer 22

goes up from left to right in a period and top to bottom in a group

Question 23

why are elements in groups 1 and 2 called the active metals

Answer 23

they are called the active metals because they have lo ionization energies

Question 24

how many electrons in groups 1 and 2 need to lose to get an octet

Answer 24

group 1 needs to lose 1; group 2, 2

Question 25

what does the number of electrons that an atom loses tell you about it

Answer 25

if it loses electrons and it gets a noble gas like electron configuration, then losing one more electron will cost much more energy

Question 26

what is electron affinity

Answer 26

electron affinity is energy disspated by a gas species when it gains an electron and is the opposite of ionization energy

Question 27

what two things determine how big the energy release will be when an atom gets an electron, in regards to electron affinity
how does electron affinity increase in groups and periods

Answer 27

the stronger the electrostatic pull or the higher the zeff between the nucleus and the valence electrons, the greater the energy the release will be when an atom gets an electron
electron affinity increases from left to right and goes down from top to bottom

Question 28

describe the trend of electron affinity for elements in groups 1 and 2 and for the halogens

Answer 28

its low in the groups 1 and 2 and prefer to give up electrons to get the octet of the noble gas in the previous period
its high in the halogens becuz they only need to get one electron to have an octet like the noble gas in the same period

Question 29

why is the electron affinity of the noble gas on the order of zero

Answer 29

becuz they already have an octet and cannot readily accept an electron

Question 30

what is electronegativity

Answer 30

its a measure of an attractive force that an atom will have an electron in a chemical bond and the greater it is the more it attracts electrons inside the bond

Question 31

how do ionization energy and electronegativity relate

Answer 31

the lower the IE, the lower the elecneg

Question 32

what elements have the least and most electronegativity and what are their values on the pauling scale
how does elec neg increase

Answer 32

0.7 for Cs, 4.0 for F

it increases from left to right and bottom to top

Question 33

Describe periodic trends in a shorthand style

Answer 33

Left to right:
Atomic radius dec
IE inc
Elec aff inc
elecneg inc

top to bottom
Atomic radius inc
IE dec
Elec aff dec
elecneg dec                 *atomic radius is always opposite the other trends

Question 34

what metals have the lowest densities

what results when group 1 metals react with water

Answer 34

alkali metals

forms strong bases

Question 35

compare the atomic radii and effective nuclear charge of group 1 and 2 metals

Answer 35

group 2 metals have a higher zeff and a slightly smaller atomic radii

Question 36

what are the elements in group 6a called and how many electrons do they have
what is the size of their atomic and ionic radii

Answer 36

they are called chalcogens and they have 6 valence electrons

they are small and large

Question 37

what are the states of matter of the halogens

Answer 37

gas f2 CL2
LIQUID BR2
SOLID I2

Question 38

frequencies not absorbed are called

and what we see is absorbed or reflected

Answer 38

subtraction frequencies

what we see is reflected