electronic and periodic properties of elements: concepts and vocab

Question 1

polyelectronic atoms

Answer 1

atoms with more than one elctron

Question 2

when “l” is 0, orbitals are in letter

Answer 2

s

Question 3

when “l” is 1, orbitals are in letter

Answer 3

p

Question 4

when “l” is 2, orbitals are in letter

Answer 4

d

Question 5

when “l” is 3, orbitals are in letter

Answer 5

f

Question 6

variations in nuclear charge and number of electrons…

Answer 6

change the magnitudes of the electrical forces that hold electrons in their orbitals

Question 7

higher nuclear charge…

Answer 7

attracts electrons more strongly

Question 8

shielding effect

Answer 8

electrons are shielded from the nuclear charge by repulsion of other electrons

Question 9

penetration effect

Answer 9

electrons in the 2s orbital are more strongly attracted to the nucleus than electrons in the 2p orbital; 2s orbital is lower energy than 2p orbital

Question 10

Z of eff

Answer 10

effective nuclear charge; attractive charge felt by valence electrons

Question 11

to calculate Z of eff

Answer 11

atomic number (#p+) - inner core of shielding electrons

Question 12

electron configuration

Answer 12

arrangement of electrons in orbitals of an atom

Question 13

what are the parts of an electron configuration symbol

Answer 13

1. number of principle quantum shell
2. letter that designated orbital type
3. superscript for number of electrons in the shell

Question 14

aufbau principle

Answer 14

as protons are added to the nucleus one by one to build up elements, electrons are similarly added to hydrogen-like orbitals

Question 15

guidelines for atomic ground states (minus orbital capacities)

Answer 15

1. each electron in an atom occupies most stable available orbital
2. no two electrons can have identical descriptions
3. higher n, less stable orbital
4. for equal n, the higher l, the less stable orbital

Question 16

hund’s rule

Answer 16

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the pauli principle in a particular set of degenerate (same energy) orbitals

Question 17

guidelines for electron configurations

Answer 17

1. each arrow represents an electrons
2. spread arrow across all the boxes before doubling up

Question 18

valence electrons

Answer 18

electrons int he outermost principle quantum level of atom

Question 19

elements in the same group…

Answer 19

have the same valence electron configuration

Question 20

electron configuration shortcut

Answer 20

go to the row above the element whose electron configuration you want to find, find the element at the end of this row and configure until reaching th desired element. write the configuration as [shortcut element] followed by the additional configuration

Question 21

in transition metal atoms

Answer 21

the ns orbital is more stable

Question 22

in transition metal cations

Answer 22

the (n-1)d orbitals are more stable

Question 23

all valence electrons in transition metals

Answer 23

occupy (n-1)d orbitals

Question 24

paramagnetic atoms/ions

Answer 24

have at least one unpaired electron, net spin, and are attracted by a strong magnet

Question 25

diamagnetic atoms/ions

Answer 25

have no unpaired electrons, no net spin, and aren’t attracted by magnets

Question 26

excited states

Answer 26

a new electron configuration an atom adopts after absorbing energy

Question 27

isoelectronic

Answer 27

atoms and ions that have the same number of electrons

Question 28

atomic radius periodic trend

Answer 28

increases from right to left and top to bottom

Question 29

why does atomic radius decrease from left to right

Answer 29

effective nuclear charge increases so valence electrons are drawn closer to the nucleus, decreasing the atoms size

Question 30

the atomic radius of cations is

Answer 30

smaller than that of its neutral atom

Question 31

the atomic radius of an anion is

Answer 31

larger than that of its neutral atom

Question 32

ionization energy

Answer 32

energy required to remove an electron from a gaseous atom or ion

Question 33

ionization energy & core electron relationship

Answer 33

core electrons are bound tighter to the nucleus than valence electrons so it takes more energy to remove them from an atom

Question 34

ionization energy periodic trend

Answer 34

increases from left to right and bottom to top

Question 35

electron affinity

Answer 35

energy change associated with addition of electrons to gaseous atoms

Question 36

electron affinity periodic trend

Answer 36

increases from left to right, decreases from top to botom/when going down a group

Question 37

metallic periodic trend

Answer 37

increases from top to bottom and right to left

Question 38

group IA ion

Answer 38

1+

Question 39

group

Question 40

to calculate the combining ratio of an ion and anion

Question 41

an anion and cation from a compound when

Answer 41

they neutralize each other/cancel out to equal 0

Question 42

to calculate the valence electrons in an element

Answer 42

t