Unit 1: Atomic Structure, Periodicity, Trends on the Periodic Table

Question 1

Allotropes

Answer 1

2 versions of the same element

Question 2

Protons

Answer 2

Charge: +1
Mass: 1
Location: Nucleus

Question 3

Neutrons

Answer 3

Charge: 0
Mass: 1
Location: Nucleus

Question 4

Electrons

Answer 4

Charge: -1
Mass: 0
Location: Valence shells

Question 5

Atomic mass =

Answer 5

fractional abundance x mass number

Question 6

Mass spectrometer

Answer 6

seperates atoms by mass

Question 7

n is the?

Answer 7

principle energy level

Question 8

Number of electrons in each level

Answer 8

2n^2

Question 9

sublevel: S

Answer 9

holds 2 electrons, 1 orbital, sphere

Question 10

sublevel: P

Answer 10

holds 6 electrons, 3 orbitals, teardrops

Question 11

sublevel: D

Answer 11

holds 10 electrons, 5 orbitals

Question 12

sublevel: F

Answer 12

holds 14 electrons, 7 orbitals

Question 13

electrons in orbitals…..

Answer 13

have different spins ↑↓

Question 14

ground state

Answer 14

as close to the nucleus as an electron can get

Question 15

Aufbau principle

Answer 15

another way to put the electron configuration in order

Question 16

electron configuration shortcut

Answer 16

go to the nearest noble gas
e.g. [Ar] 4s2 3d10 4p3

Question 17

what type of sublevels are more stable?

Answer 17

half-filled sublevels and full sublevels

Question 18

isoelectronic

Answer 18

‘same configuration’

Question 19

c=λv

Answer 19

c: speed of light
λ: wavelength
v: frequency

Question 20

E=hv

Answer 20

Equation for the incoming energy of electromagnetic radiation
E: energy
h: planck’s constant
v: frequency

Question 21

Longer wavelengths have….

Answer 21

lower frequency

Question 22

Shorter wavlengths have….

Answer 22

higher frequency

Question 23

Periodicity

Answer 23

repeating patterns of physical and chemical properties

Question 24

Metals tend to….

Answer 24

lose electrons

Question 25

Non-metals tend to….

Answer 25

gain electrons

Question 26

Atomic radius trend

Answer 26

increases down and to the left, focuses on electrons

Question 27

Shielding

Answer 27

increases down and to the right, focuses on protons

Question 28

1st ionization energy

Answer 28

energy to remove an electron, increases up and to the right

Question 29

Electronegativity

Answer 29

attraction an atom has for the electrons in a bond, closest to Fluorine in the most electronegative, increases up and to the right, covalent < 1.7 < ionic

Question 30

Electron affinity

Answer 30

energy released when one electron is added to a neutral atom in the gas state (exothermic), adding second electron is endothermic, increases up and to the right

Question 31

Melting point

Answer 31

transition metals have a high melting point, metaks have a low melting point, carbon’s family has a high melting point, diamond has the highest melting point.
The more metals in the valence, the harder the metals, the higher the metling point.

Question 32

Basic oxides

Answer 32

Metals: tend to lose electrons, tend to be ionic oxides

Question 33

Acidic oxides

Answer 33

Non-metals: tend to gain electrons, tend to be covalent oxides

Question 34

Amphoteric

Answer 34

it acts as a base in some situations and an acid in others - e.g. Al2O3

Question 35

Transition metals

Answer 35

incomplete ‘d’ sublevel, Zn is an exception

Question 36

Variable oxidation states

Answer 36

just a broader term for the charge

Question 37

Ligands

Answer 37

complex ions, ligands are lewis bases, metal ions are lewis bases, lewis acid recieves the lone pair, lewis base provides the lone pair, must use square brackets for complex ions

Question 38

Coordinate covalent bond

Answer 38

one atom provides both electrons for covalent bonds

Question 39

Dimagentism

Answer 39

only paired electrons, commonly ‘non-magnetic’, weak repulsion in a magnetic field

Question 40

Paramagnetism

Answer 40

half-filled orbitals, the more half-filled orbitals the more magnetic, strong repulsion in a magnetic field

Question 41

Ferromagnetism

Answer 41

lots of half-filled orbitals, everday magnetism, Fe, Co, Ni

Question 42

Catalyst

Answer 42

something that causes a reaction to go faster, increases reaction rate, the catalyst is unchanged during the reaction

Question 43

Heterogeneous

Answer 43

transition metals

Question 44

Homogeneous

Answer 44

enzymes, Iron (II), Cobalt (III)

Question 45

Colorwheel

Answer 45

transition metals often have bright colors, complimentary colors are opposite, Sc3+ is colorless (there are no electrons in a d sublevel)

Question 46

Photons of visible light can….

Answer 46

promote (raise) an electron to a slightly higher energy level

Question 47

4 factors

Answer 47

identity of a ligand, identity of the metal ion, geometry, oxidation state on the metal ion

Question 48

LEO says GER

Answer 48

LEO: loss of electrons, oxidation - reducing agent, causes reduction
GER: gain of electrons, reduction - oxidizing agent, causes oxidation