Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

IB Chemistry > deck_17051147 > Flashcards

deck_17051147 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

How are groups arranged on the P.T.?

A

They go down

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Group 1

A

Alkali Metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Group 2

A

Alkali Earth Metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Groups 3-12

A

Transition Metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Group 17

A

Halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Group 18

A

Noble Gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How are periods arranged on the P.T?

A

They go across left to right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What do periods correspond with?

A

The number of Principle Energy Levels where valence electrons are located

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Where are Metals located?

A

Left of Staircase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What do Metals form?

A

Cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Description of metals

A

Malleable, ductile, good conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Where are nonmetals located?

A

Right of the staircase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What do nonmetals form?

A

Anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Description of nonmetals

A

Brittle, dull, non-conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Locations of metalloids

A

Touch the staircase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the metalloids?

A

B, Si, Ge, As, Sb, Te

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Nuclear Charge

A

Represented by atomic number and increases by one through each successive element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

The outer electrons determine what?

A

Many physical and chemical properties of an element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What prevents the valence electrons from experiencing the full nuclear charge?

A

Repulsion and Shielding due to the inner electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

As you go across period…

A
  1. Same amount of shielding
  2. Greater nuclear charge
    More effective nuclear charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

As you go down group…

A
  1. Same effective nuclear charge
  2. Charge increases by 8
  3. Shielding increases by 8
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Atomic Radius

A

Half the distance between neighboring atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Why does atomic radius increase down a group?

A

Greater numbers of P.E.L.’s as seen by period number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why does atomic radius decrease across a period?

A

Same number of P.E.L.’s, greater nuclear charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Cations are ___ than its atom

A

Smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Anions are ___ than its atom

A

Larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Isoelectronic

A

The same electronic configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Cations have a…

A

Greater nuclear charge which pulls electrons closer, have a smaller radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Anions have a…

A

Smaller nuclear charge, cannot pull electrons as close, larger radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Electron Affinity

A

A measure in the charge in energy when one mole of its electrons are added to one mole of gaseous atoms to form gaseous ions; exothermic process
Becomes endothermic when adding a second electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Electronegativity

A

A measure of an element’s attraction for one electron in a covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Electronegativity increases…

A

Across a period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Electronegativity decreases…

A

Down a group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

The melting point of metals…

A

Increases as the number of valence electrons increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Metalloids have…

A

Very high melting points and strong bonds due to being covalent structures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

The melting point of nonmetals…

A

Are low due to weak intermolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

The melting point of Noble Gases…

A

Are very low due to very weak intermolecular forces and being monatomic

38
Q

Chemical properties of metals

A

-More reactive as you go down groups
-React by losing electrons
-Bigger, easier to lose electrons

39
Q

Metal Oxides with Acids

A

Form a salt and water
Neutralization reaction, the metal cation bonds with the acidic anion to form a salt, the leftover H and O form water

40
Q

Nonmetal Oxides with Bases (Alkali)

A

Form a salt and water
Neutralization reaction, shows that nonmetal Oxides are acidic in nature

41
Q

Group 17 Reactivity

A

Most reactive at the top (F)

42
Q

Properties of Fluorine

A

Yellow gas

43
Q

Properties of Chlorine

A

Yellow/green gas

44
Q

Properties of Bromine

A

Dark Red liquid

45
Q

Properties of Iodine

A

Purple Solid

46
Q

Displacement reaction

A

A more reactive halogen will be in compound form, less reactive alone

47
Q

Nonmetal Oxides in water

A

Bonds together, forms an acid

48
Q

Amphoteric Oxide (Al2O3)

A

Can act as both an acid and base (Lewis)

49
Q

What two Nonmetal Oxides do not react with water?

A

SiO2 and CO

50
Q

Properties of Transition Metals

A
  1. Variable oxidation states
  2. Incomplete d sublevel as atom or as positive ion
  3. Catalytic and magnetic properties
  4. Form complex ions with ligands
  5. Colored compounds
51
Q

How is Zinc not a Transition Metal

A

It always has a complete d sublevel, is always colorless and only has one oxidation state

52
Q

All Transition Metals can form what two oxidation states?

A

+2 and +3

53
Q

From Sc to Cr, what oxidation state is the most common?

A

+3

54
Q

The +2 oxidation state is most common where?

A

After Mn due to a greater nuclear charge making it harder to lose more than two electrons

55
Q

Where and what is the maximum oxidation state?

A

At Mn, highest is +7

56
Q

Trend for oxidation states

A

Oxidation states increase by one up to Mn, where they decrease by one after

57
Q

What two metals have the highest oxidation states and are the best oxidizing agents?

A

Mn +7 and Cr +6

58
Q

What do Transition Metals do as catalysts?

A

Increase the rate of reaction and provide an alternate pathway

59
Q

Homogeneous catalyst

A

A catalyst in the same phase as the reactant(s)

60
Q

Medical uses of Transition Metals

A
  1. Fe +2 heme in blooded to transport oxygen
  2. Co +3 in vitamin B12
61
Q

Heterogeneous Catalyst

A

A catalyst in a different phase than the reactant(s)

62
Q

Catalyst Converter

A

(Pd/Pt catalysts) Converts CO and NO into CO2 and N2
2CO + 2NO = 2CO2 and N2

63
Q

Haber Process

A

(Fe catalyst) The production of ammonia from its elements
N2 + 3H2 = 2NH3

64
Q

Contact Process

A

(V2O5 Vanadium V Oxide Catalyst) Production of sulfuric acid
2SO2 + O2 = 2SO3

65
Q

Hydrogenation

A

(Ni catalyst) Converting unsaturated hydrocarbons into saturated hydrocarbons
C2H4 + H2 = C2H6

66
Q

Decomposition of Hydrogen Peroxide

A

(MnO2 catalyst) 2H2O2 = 2H2O + O2

67
Q

Magnetic properties of Transition metals

A

How they behave when introduced to a magnetic field

68
Q

Paramagnetic

A

Contains unpaired electrons
-Will be pulled into a magnetic field
-Do not retain magnetic properties
-More unpaired electrons, more attraction

69
Q

Diamagnetic

A

Contains paired electrons
-Weakly repelled by magnetic properties after field is removed

70
Q

Ferromagnetic

A

Contain unpaired electrons that align parallel to each other in domains
-Retain magnetic properties when magnetic field is removed (Iron, Cobalt, Nickel)

71
Q

Complex Ion

A

Because of their small size, d block ions act as Lewis acids and attract species that are electron rich (ligands)

72
Q

Ligands

A

Species with lone pair(s) of electrons that form coordinate covalent bonds with a central metal ion. Ligands are Lewis bases

73
Q

Spectrochemical series

A

I - < Br - < S -2 < F - < OH - < SCN- < NH3 < CO = CN -
Weakest -> strongest
Stronger = more splitting

74
Q

Monodetant ligands

A

Form one coordinate covalent bond using one lone pair of electrons
*If the ligand is neutral, the charge of the central ion is the same as the complex ion
*The number of coordinate covalent bonds from the ligand to the central ion is the coordination number

75
Q

Polydentant Ligands

A

Contain more than one pair of lone electrons and can form two or more coordinate covalent bonds to the central ion

76
Q

Bidentant Ligands

A

Can form two coordinate covalent bonds (Oxalate ion C2O4 -2)

77
Q

Ethylenediamine

A

H2NCH2CH2NH2

78
Q

Hexadentate ligand

A

Has six atoms with lone pairs of electrons (EDTA -4)

79
Q

Chelate

A

Two or more separate coordinate covalent bonds between ligand and central atom

80
Q

Oxidization rules

A
  1. Compounds sum to zero
  2. Ions sum out to their charge (NO3-)
  3. Lone elements = 0
  4. Group 1 metals = +1
  5. Group 2 metals = +2
  6. Oxygen is almost always -2, unless peroxide or with F-2
  7. Hydrogen is +1 unless with metal -1
  8. Fluorine is always -1
81
Q

Oxidation states vs oxidation numbers

A

Oxidation states: (+) or (-) in front
Oxidation numbers: Roman numerals

82
Q

Color of Transition Metals

A

-Related to presence of partially filled d orbitals
-The color is determined by the color of light it absorbs and which color it transmits or reflects (Opposite color on the color wheel)

83
Q

Degenerate

A

A free ion, the d orbitals are all of equal energy

84
Q

Location of the 5 d orbitals

A

3 between the axis
2 along the axis

85
Q

Splitting

A

When a ligand comes in, its lone electrons repell the 2 orbitals along the axis, causing them to split, anything that changes the splitting changes the color

86
Q

Identity of central metal ion

A

-Larger metals provide greater splitting
-A greater nuclear charge will cause a greater electrostatic attraction to the ligand and result in more splitting
More energy = more splitting

87
Q

Oxidation state of metal ion

A

As oxidation state increases for the same metal, the splitting of the d orbitals also increases

88
Q

Geometry of Complex ion

A

Octahedrall (6) > Tetrahedral (4) > Linear (2)

89
Q

Identity of ligand

A

Stronger ligand = greater splitting

90
Q

(Cu(H2O)6) vs [Cu(NH3)4(H2O)2]

A

When some of the water ligands are replaced by ammonia the splitting of the d orbital increases. The new complex Ion will absorb more energy and light with decreasing wavelength.

IB Chemistry (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions