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general chemistry > Periodic Table Trends > Flashcards

Periodic Table Trends Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

ionic radii trends

A

decreases from left to right
increases down a group

ionic radii decreases as atomic number increases

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2
Q

cations

A

positively charged

usually smaller because less electrons

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3
Q

anions

A

negatively charged

usually larger because more electrons

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4
Q

Effective Nuclear Charge

A

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

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5
Q

What happens to the Zeff with more electrons

A

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

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6
Q

What happens to Zeff with less electrons

A

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

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7
Q

chalcogens

A

oxygen group

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8
Q

pnictogens

A

nitrogen group

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9
Q

elements in same group

A

have same number of electrons

same chemical properties, different physical properties

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10
Q

diatomic atoms

A

form double covalent bonds to achieve full valence shell of electrons

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
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11
Q

strong Lewis acids

A

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

want small ionic radius and large positive charge

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12
Q

strong Lewis base

A

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

lower electronegativity (more easily give up electrons)

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13
Q

metals

A

low electronegativity and low ionization energy

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14
Q

ionization energy

A

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

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15
Q

diamagnetics

A

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

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16
Q

paramagnetic

A

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

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17
Q

Pauli Exclusion Principle

A

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

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18
Q

Hund’s Rule

A

maximize the number of unpaired electrons

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

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19
Q

Polarizability

A

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

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20
Q

electron affinity

A

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

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21
Q

electronegativity

A

tendency to attract electrons within a bond

increases moving across and up the periodic table

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22
Q

ionization energy

A

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

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23
Q

first ionization energy

A

energy required to remove the first valence electron of

24
Q

second ionization energy

A

energy required to remove the second valence electron

25
Q

which group has the lowest first ionization energy

A

alkali metals - group 1

because only has one electron that they really want to remove

26
Q

which group has the lowest second ionization energy

A

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

27
Q

isotopes

A

atoms of the same element with different number of neutrons

designated by their mass number

28
Q

How to find number of neutrons

A

mass number - atomic number

29
Q

atomic number

A

number of protons

determines identity of an element

30
Q

atomic mass number

A

amu is in terms of carbon-12
sum of protons and neutrons

1 mol amu = 1 g = 6.02 x 10^23 amu

31
Q

sp

A

linear

180 degrees

32
Q

sp2 - no lone pairs

A

trigonal planar

120 degrees

33
Q

sp3 - no lone pairs

A

tetrahedral

109 degrees

34
Q

sp3d - no lone pairs

A 
trigonal bipyramidal
90 degrees (for 3)
120 degrees (for 2)
35
Q

sp3d2 - no lone pairs

A

octahedral

90 degrees

36
Q

what hydridization is the most electronegative?

A

the more s character, the more electronegative

sp is the most electronegative

37
Q

sp2 - one lone pair

A

bent

117.5 degrees

38
Q

sp3 - one lone pair

A

trigonal pyramidal

107.3 degrees

39
Q

sp3 - two lone pairs

A

bent

104 degrees

40
Q

sp3d - one lone pair

A

sawhorse

41
Q

sp3d - two lone pairs

A

T-shaped

42
Q

sp3d - three lone pairs

A

linear

43
Q

sp3d2 - one lone pair

A

square pyramidal

44
Q

sp3d2 - two lone pairs

A

square planar

45
Q

sp3d2 - three lone pairs

A

T-shaped

46
Q

sp3d2- four lone pairs

A

linear

47
Q

metals

A

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

48
Q

nonmetals

A

poor conductors, high electronegativity, unwilling to part with electrons

49
Q

bond strength

A

decreases moving down the periodic table as acidity increases

because the larger the molecules get, the harder to hold together

50
Q

acidity

A

the more electronegative something is, the more acidic

51
Q

electron affinity

A

increases toward more electronegative elements

decreases moving down a column because the charge becomes more spread out

inversely related to atomic radius

52
Q

ionization energy

A

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

53
Q

What more effectively decides atomic radius?

A

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

54
Q

orbitals of water?

A

104.5 degree angle because lone pairs affect angles

55
Q

What groups contain the longest bond lengths?

A

increasing atomic radius

56
Q

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

A

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

57
Q

How to determine which is the lower energy of a subshell

A

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

general chemistry (10 decks)

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