chp 5 test

Question 1

alkali metals properties (group 1)

Answer 1

highly reactive

not found isolated in nature

Question 2

alkaline-earth elements properties (group 2)

Answer 2

metals

highly reactive

Question 3

transition elements properties (groups 3-12)

Answer 3

metals
good conductors
reactivity varies

Question 4

metals properties (groups 3-16)

Answer 4

reactive

Question 5

metalloids properties (groups 3-16)

Answer 5

some properties of metals/ some properties of nonmetals

semiconductors

Question 6

nonmetals properties (groups 3-16)

Answer 6

C, N, O, P, S

primary components of living things

Question 7

halogens properties (group 17)

Answer 7

most reactive nonmetals

Question 8

noble gases properties (group 18)

Answer 8

nonreactive

Question 9

lanthanides properties (top bottom row)

Answer 9

metals

Question 10

actinides properties (bottom bottom row)

Answer 10

tend to be radioactive

some actinides are man made

Question 11

ionization energy

Answer 11

the energy required to remove one electron from an atom

Question 12

IE equation

Answer 12

A + energy —> e- + A+

Question 13

highest and lowest IE

why?

Answer 13

highest: group 18
because it has a full octet and is already stable so more energy is required to break up the octet

lowest: group 1
because the elements become more stable by losing an electron

Question 14

IE trend down a group

why?

Answer 14

as you move down a group, IE decreases

because the electron being removed is further from the positive nucleus

Question 15

second ionization energy

Answer 15

the energy required to remove the second electron from an atom

Question 16

second IE equation

Answer 16

A+ + energy —> e- + A2+

Question 17

highest and lowest second IE

why?

Answer 17

highest: group 1
because they have an octet of electrons after leaving 1e-

lowest: group 2
because they obtain an octet by losing 2e-

Question 18

third ionization energy

Answer 18

the energy required to remove the third electron from an atom

Question 19

third IE equation

Answer 19

A2+ + energy —> e- + A3+

Question 20

highest and lowest third IE

why?

Answer 20

highest: group 2
because they have an octet after losing 2e-

lowest: group 3
because they achieve an octet by losing 3e-

Question 21

electron affinity

Answer 21

the energy charge that occurs when an atom gains an electron

Question 22

positive EA

Answer 22

energy is required for an atom to gain the electron

Question 23

negative EA

Answer 23

energy is released as the atom gains the electron

Question 24

positive EA equation

Answer 24

A + e- + energy—> A-

Question 25

negative EA equation

Answer 25

A + e- —> A- + energy

Question 26

highest positive EA | why?

Answer 26

group 18 | because they have an octet of electrons

Question 27

highest negative EA | why?

Answer 27

group 17 | because they become more stable by gaining 1e-

Question 28

electronegativity

Answer 28

a measure of the ability of an atom in a chemical compound to attract electrons

Question 29

highest and lowest EN | why?

Answer 29

highest: group 17 because they become more stable by gaining electrons lowest: group 1 because they become more stable by losing electrons

Question 30

noble gases (group 18) EN

Answer 30

do not have EN values because they do not form compounds

Question 31

atomic radius trend down a group | why?

Answer 31

as you move down a group, the atomic radius increases | because new energy levels of electrons are added

Question 32

atomic radius trend across a group | why?

Answer 32

as you move across a group, the atomic radius decreases because no new energy levels are added, the nuclear charge increases, and electrons are being pulled closer to the nucleus

Question 33

cation

Answer 33

positive ion

Question 34

anion

Answer 34

negative ion

Question 35

cation size compared to neutral atom | why?

Answer 35

always smaller than their neutral atoms | because the same nuclear charge is exerted on fewer electrons

Question 36

anion size compared to neutral atom | why?

Answer 36

always larger than their neutral atoms | because the same nuclear charge is exerted on more electrons