Periodic Table Trends

Question 1

ionic radii trends

Answer 1

decreases from left to right
increases down a group

ionic radii decreases as atomic number increases

Question 2

cations

Answer 2

positively charged

usually smaller because less electrons

Question 3

anions

Answer 3

negatively charged

usually larger because more electrons

Question 4

Effective Nuclear Charge

Answer 4

the net positive charge felt by an electron in an atom

the shielding effect of negatively charged electrons prevents higher orbital electrons from experiencing the full nuclear charged of the nucleus due to the repelling effect of inner-layer electrons

Question 5

What happens to the Zeff with more electrons

Answer 5

the more electrons you have will increase electronic repulsion and nuclear shielding which will decease Zeff

Question 6

What happens to Zeff with less electrons

Answer 6

less electrons means electrons get pulled closer to the nucleus which increases Zeff

Question 7

chalcogens

Answer 7

oxygen group

Question 8

pnictogens

Answer 8

nitrogen group

Question 9

elements in same group

Answer 9

have same number of electrons

same chemical properties, different physical properties

Question 10

diatomic atoms

Answer 10

form double covalent bonds to achieve full valence shell of electrons

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine

Question 11

strong Lewis acids

Answer 11

want to accept electrons
strength will increase with increasing ionic charge and decreasing ionic radius

want small ionic radius and large positive charge

Question 12

strong Lewis base

Answer 12

wants to donate electrons
highly negative with lots of lone pair electrons

lower electronegativity (more easily give up electrons)

Question 13

metals

Answer 13

low electronegativity and low ionization energy

Question 14

ionization energy

Answer 14

the amount of energy required to remove an electron from a neutral atom

Question 15

diamagnetics

Answer 15

no unpaired electrons

slightly repels magnets
goes against the magnetic field
parallel spin alignment
slightly bends away from field

ex: Noble gases or ions with complete pairings due to losing electrons

Question 16

paramagnetic

Answer 16

has unpaired electrons which can interact with a magnetic field

attracted to magnets
aligned with magnetic field
anti-parallel spin alignment
magnetic field lines bend toward it

good MRI contrasting agent by enhancing signal in tissues

Question 17

Pauli Exclusion Principle

Answer 17

each orbital can hold a max of 2 electrons, with opposite spin

Question 18

Hund’s Rule

Answer 18

maximize the number of unpaired electrons

- want to fill up every orbital in a sublevel with one electron before pairing

Question 19

Polarizability

Answer 19

extent to which an electron cloud of an atom can be distorted by an external charge or by an applied electric field to produce a dipole

Question 20

electron affinity

Answer 20

measure of tendency of atom to accept electrons
will increase moving across and up the periodic table

a negative value means more likely to accept electrons

Question 21

electronegativity

Answer 21

tendency to attract electrons within a bond

increases moving across and up the periodic table

Question 22

ionization energy

Answer 22

opposite of electron affinity
measures energy required to remove an electron from an atom

increases with increasing atomic radius because the electrons are more dispersed and easier to remove

Question 23

first ionization energy

Answer 23

energy required to remove the first valence electron of

Question 24

second ionization energy

Answer 24

energy required to remove the second valence electron

Question 25

which group has the lowest first ionization energy

Answer 25

alkali metals - group 1 | because only has one electron that they really want to remove

Question 26

which group has the lowest second ionization energy

Answer 26

alkaline earth metals - group 2 because have 2 electrons that they want to get rid of not alkali metals because they only have 1 valence electron to give and then will have to dip into core electrons which require a lot more energy

Question 27

isotopes

Answer 27

atoms of the same element with different number of neutrons | designated by their mass number

Question 28

How to find number of neutrons

Answer 28

mass number - atomic number

Question 29

atomic number

Answer 29

number of protons | determines identity of an element

Question 30

atomic mass number

Answer 30

amu is in terms of carbon-12 sum of protons and neutrons 1 mol amu = 1 g = 6.02 x 10^23 amu

Question 31

sp

Answer 31

linear | 180 degrees

Question 32

sp2 - no lone pairs

Answer 32

trigonal planar | 120 degrees

Question 33

sp3 - no lone pairs

Answer 33

tetrahedral | 109 degrees

Question 34

sp3d - no lone pairs

Answer 34

``` trigonal bipyramidal 90 degrees (for 3) 120 degrees (for 2) ```

Question 35

sp3d2 - no lone pairs

Answer 35

octahedral | 90 degrees

Question 36

what hydridization is the most electronegative?

Answer 36

the more s character, the more electronegative sp is the most electronegative

Question 37

sp2 - one lone pair

Answer 37

bent | 117.5 degrees

Question 38

sp3 - one lone pair

Answer 38

trigonal pyramidal | 107.3 degrees

Question 39

sp3 - two lone pairs

Answer 39

bent | 104 degrees

Question 40

sp3d - one lone pair

Answer 40

sawhorse

Question 41

sp3d - two lone pairs

Answer 41

T-shaped

Question 42

sp3d - three lone pairs

Answer 42

linear

Question 43

sp3d2 - one lone pair

Answer 43

square pyramidal

Question 44

sp3d2 - two lone pairs

Answer 44

square planar

Question 45

sp3d2 - three lone pairs

Answer 45

T-shaped

Question 46

sp3d2- four lone pairs

Answer 46

linear

Question 47

metals

Answer 47

good conductors of heat, malleable & ductile, easily gives up electrons

Question 48

nonmetals

Answer 48

poor conductors, high electronegativity, unwilling to part with electrons

Question 49

bond strength

Answer 49

decreases moving down the periodic table as acidity increases because the larger the molecules get, the harder to hold together

Question 50

acidity

Answer 50

the more electronegative something is, the more acidic

Question 51

electron affinity

Answer 51

increases toward more electronegative elements decreases moving down a column because the charge becomes more spread out inversely related to atomic radius

Question 52

ionization energy

Answer 52

follow same pattern as electronegativity are the hardest to remove electrons from as we move down a column, the radius will increase which decreases the intermolecular forces, making it easier to remove electron because not bound as tightly

Question 53

What more effectively decides atomic radius?

Answer 53

because addition of shells has a strong effect on shielding, changes in atomic radius down a group are more pronounced than for those across a period

Question 54

orbitals of water?

Answer 54

104.5 degree angle because lone pairs affect angles

Question 55

What groups contain the longest bond lengths?

Answer 55

increasing atomic radius

Question 56

How to determine which level of electron configuration an electron is removed from

Answer 56

if have a positive cation like Cu2+ --> will remove from the highest value for "n" and if they are tied then the highest "l" ex: Osmium is [Xe]6s^2 4f^14 5d^6 if we removed 2 electrons - they would come from s group because it has the highest "n" value at 6. If there was a p group - would remove from p because they have the same "n" but p has L=1 vs s=0

Question 57

How to determine which is the lower energy of a subshell

Answer 57

n+l rule s=0 p=1 d=2 f=3 ex: 5d vs 6s ``` 5d = 5+2 = 7 6s = 6+0 = 6 ``` the lower energy is 6s and therefore the electrons would be added there first