The Periodic Table

Question 1

rows of elements, 1-7, represent principal quantum number (n)

Answer 1

periods

Question 2

columns of elements, 1-18 or IA-VIIIA and IB-VIIIB

Answer 2

groups

Question 3

left side and middle of periodic table; they are lustrous, malleable, ductile; easily give up electrons; good conductors

Answer 3

metals

Question 4

at atomic level: low effective nuclear charge (Zeff), low electronegativity, large atomic radius, small ionic radius, low ionization energy, low electron affinity

Answer 4

metals

Question 5

upper right of periodic table; brittle and show little luster in solid state; poor conductors, do NOT easily give up electrons

Answer 5

nonmetals

Question 6

at atomic level: high ionization energies, high electron affinities, high electronegativities, small atomic radii, large ionic radii

Answer 6

nonmetals

Question 7

stair step group separating metals and nonmetals, they share characteristics of each; elements include: B, Si, Ge, As, Sb, Ge, Po, At

Answer 7

metalloids

Question 8

electrostatic attraction between valence shell electrons and nucleus, measure of net positive charge experienced by outermost electrons;
trend: increases to the right, remains relatively constant between periods

Answer 8

effective nuclear charge (Zeff)

Question 9

elements with a stable octet of valence electrons, group VIIIA or 18

Answer 9

noble (inert) gases

Question 10

size of a neutral element;

trend: increases down and to the left, opposite of all other trends

Answer 10

atomic radius

Question 11

dependent on how element ionizes based on type and group number; cations are generally smaller, anions are generally larger

Answer 11

ionic radius

Question 12

energy required to remove an electron from a gaseous species, requires input of heat (endothermic process);
trend: increases up and to the right, IE 1 < IE 2 < IE 3 …;
univalent cation: X+
diavalent cation: X2+

Answer 12

ionization energy (IE)

Question 13

energy dissipated by a gaseous species when it gains an electron (exothermic process);
trend: increases up and to the right

Answer 13

electron affinity

Question 14

measure of attractive force that an atom will exert on an electron in a chemical bond;
trend: increases up and to the right

Answer 14

electronegativity

Question 15

group IA (1), one valence electron

Answer 15

alkali metals

Question 16

group IIA (2), two valence electrons

Answer 16

alkaline earth metals

Question 17

alkali metals and alkaline earth metals are considered…

Answer 17

active metals

Question 18

VIA (16), not as reactive as halogens but crucial for biological functions, six valence electrons

Answer 18

chalcogens

Question 19

VIIA (17), highly reactive nonmetals, seven valence electrons

Answer 19

halogens

Question 20

VIIIA (18), minimal reactivity, eight valence electrons = filled valence shell (full octet)

Answer 20

noble (inert) gases

Question 21

groups IB to VIIIB (3-12), contains metals, many can have oxidation states

Answer 21

transition metals

Question 22

different possible charged forms of elements because capable of losing different numbers of electrons from s and d orbitals in their valence shells, different states often correspond to different colors

Answer 22

oxidation states