Periodic Table

Question 1

cation

Answer 1

postive charge

Question 2

anion

Answer 2

negative charge

Question 3

period

Answer 3

rows in p table

Question 4

group

Answer 4

columns in p table

Question 5

orbital

Answer 5

the region in an atom where an electron is likely to be found, 2 electrons per orbital

Question 6

sublevel

Answer 6

a set of electrons having the same energy

Question 7

energy level

Answer 7

a fixed distance from the nucleus where electrons can be found (discrete levels, not continuous)

Question 8

hund’s rule

Answer 8

all orbitals in a sublevel must have 1 electron before any have 2

Question 9

pauli exclusion principle

Answer 9

orbitals can’t have more than two electrons, they must be opposite spins

Question 10

aufbau principle

Answer 10

lower energy levels must be filled before higher ones (diagram)

Question 11

bohr diagram

Answer 11

shows electrons in energy levels (in rings) around nucleus, can draw every electron or label inner levels with _ e

Question 12

electron configuration

Answer 12

notation to describe electrons in sublevels in an atom (ex: 1s2, 2s2, 2p4)

Question 13

electron arrangment

Answer 13

how electrons are arranged in an atom, expressed via election configuration

Question 14

orbital filling diagram

Answer 14

the diagram with boxes and arrows in different sublevels that show a visual representation of electron configuration

Question 15

coulombic attraction

Answer 15

the attraction of outer electrons to the nucleus, depends on number of protons and number of shells

Question 16

coulombic attraction pattern

Answer 16

increases across periods, decreases down groups

Question 17

electron shielding

Answer 17

core electron prevent outer electron from feeling the full force of the nucleus because electron repel each other (like a lamp shade)

Question 18

effective nuclear charge

Answer 18

net positive charge experienced by an electron (Z eff = # of protons - shielding constant)

Question 19

atomic radius

Answer 19

(bonding atomic radius) is half the distance between the nuclei of two of the same bonded atoms, in pm

Question 20

ionization energy

Answer 20

the amount of energy required to remove an electron from an atom (+KJ/mol)

Question 21

ionization energy trend

Answer 21

increase across period, decrease down groups

Question 22

electron affinity

Answer 22

(-KJ/mol) the amount of energy gained when an electron is added to an atom

Question 23

electron affinity trend

Answer 23

irregular: most in group 7, least in groups 2 and 8 (doesn’t want to add if going to another sublevel)

Question 24

reactivity

Answer 24

determined by valence electrons: groups 1 and 7 are v reactive, 8 is not

Question 25

octet rule

Answer 25

atoms gain/lose/share valence electrons to achieve full outer shell (noble gases aren’t reactive)

Question 26

alkali metals

Answer 26

group 1, highly reactive

Question 27

alkaline earth metals

Answer 27

group 2, 2 valence electrons

Question 28

transition metals

Answer 28

the d block

Question 29

halogens

Answer 29

group 17, 7 valence electrons

Question 30

post-transition metals

Answer 30

lower left p block

Question 31

non-metals

Answer 31

upper right p block (plus H), no luster, usually brittle, poor conductors, low melting point, solid, liquid, or gas, typically form anions

Question 32

metals

Answer 32

left/bottom of p table, luster, maleable, conductors, solid at room temp (varying melting points), form cations

Question 33

actinides

Answer 33

first row in f block

Question 34

lanthanides

Answer 34

second row in f block

Question 35

metallic character

Answer 35

amount an element exhibits physical/chemical properties of metal (increases down groups, decreases across periods)