Brainscape's Knowledge GenomeTM

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


See full index

A-Level Chemistry > 3.1.1 - Periodicity > Flashcards

3.1.1 - Periodicity Flashcards

1
Q

Hydrogen (H)

A

1s1

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

Helium (He)

A

1s2

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

Lithium (Li)

A

1s2, 2s1

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

Beryllium (Be)

A

1s2, 2s2

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

Boron (B)

A

1s2, 2s2, 2p1

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

Carbon (C)

A

1s2, 2s2, 2p2

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

Nitrogen (N)

A

1s2, 2s2, 2p3

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

Oxygen (O)

A

1s2, 2s2, 2p4

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

Fluorine (F)

A

1s2, 2s2, 2p5

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

Neon (Ne)

A

1s2, 2s2, 2p6

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

Sodium (Na)

A

1s2, 2s2, 2p6, 3s1

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

Magnesium (Mg)

A

1s2, 2s2, 2p6, 3s2

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

Aluminium (Al)

A

1s2, 2s2, 2p6, 3s2, 3p1

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

Silicon (Si)

A

1s2, 2s2, 2p6, 3s2, 3p2

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

Phosphorus (P)

A

1s2, 2s2, 2p6, 3s2, 3p3

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

Sulfur (S)

A

1s2, 2s2, 2p6, 3s2, 3p4

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

Chlorine (Cl)

A

1s2, 2s2, 2p6, 3s2, 3p5

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

Argon (Ar)

A

1s2, 2s2, 2p6, 3s2, 3p6

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

Potassium (K)

A

1s2, 2s2, 2p6, 3s2, 3p6, 4s1

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

Calcium (Ca)

A

1s2, 2s2, 2p6, 3s2, 3p6, 4s2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Scandium (Sc)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d1, 4s2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Titanium (Ti)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d2, 4s2

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

Vanadium (V)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d3, 4s2

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

Chromium (Cr)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s2

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

Manganese (Mn)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s2

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

Iron (Fe)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d6, 4s2

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

Cobalt (Co)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d7, 4s2

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

Nickel (Ni)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d8, 4s2

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

Copper (Cu)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2

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

Zinc (Zn)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2

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

Gallium (Ga)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p1

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

Germanium (Ge)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p2

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

Arsenic (As)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p3

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

Selenium (Se)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p4

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

Bromine (Br)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p5

36
Q

Krypton (Kr)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6

37
Q

Rubidium (Rb)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 5s1

38
Q

Strontium (Sr)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 5s2

39
Q

Yttrium (Y)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d1, 5s2

40
Q

Zirconium (Zr)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d2, 5s2

41
Q

Niobium (Nb)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d4, 5s2

42
Q

Molybdenum (Mo)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d5, 5s2

43
Q

Technetium (Tc)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d5, 5s2

44
Q

Ruthenium (Ru)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d7, 5s2

45
Q

Rhodium (Rh)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d8, 5s2

46
Q

Palladium (Pd)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2

47
Q

Silver (Ag)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2

48
Q

Cadmium (Cd)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2

49
Q

Indium (In)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2, 5p1

50
Q

Tin (Sn)

A

1s2, 2s2, 2p6, 3s2, 3p6, 3p10, 4s2, 4p6, 4d10, 5s2, 5p2

51
Q

Describe what Dimitri’s periodic table was like in 1863

A
  • 56 known elements
  • arranged in order of atomic mass
  • lined up elements of similar properties
  • predicted properties of missing elements from group trends
52
Q

Describe how the periodic table is arranged today

A
  • 118 elements
  • arranged in 7 rows (periods)
  • 18 vertical groups
  • element positions are linked to their physical and chemical properties
53
Q

across the period are _________ trend in properties of elements called ___________ (ie from metals to non-metals)

A
  • repeating
  • periodicity
54
Q

What is group 1 called?

A

Alkali metals

55
Q

What is Group 2 called?

A

Alkali earth metals

56
Q

What is Group 3-12 called?

A

Transition elements

57
Q

What is Group 15 called?

A

Pnictogens

58
Q

What is Group 16 called?

A

Chalogens

59
Q

What is Group 17 called?

A

Halogens

60
Q

What is Group 18 called?

A

Noble gases

61
Q

What does ionisation energy measure?

A

This measures how easily an atom loses electrons to form positive ions

62
Q

What is the first ionisation energy?

A

The energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

63
Q

Write the first ionisation equation for Sodium

A

Na (g) -> Na+ (g) + e-

64
Q

Factors affecting ionisation energy

A
  • atomic radius
  • nuclear charge
  • electron shielding
65
Q

How many ionisation energies does an element have?

A

An element has as many ionisation energies as there are electrons. For example, helium has 2 electrons and 2 ionisation energies.

66
Q

What is the second ionisation energy?

A

Is the energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+

67
Q

In Fluorine, why is there a large increase between the 7th and 8th ionisation energies?

A

It suggests that the eighth electron must be removed from a different shell. The first shell (n=1, closer to the nucleus) contains 2 electrons. The second shell (n=2, the outer shell) contains 7 electrons.

68
Q

Successive ionisation energies allow predictions to be made about:

A
  • the number of electrons in the outer shell
  • the group of the element in the periodic table
  • the identity of an element
69
Q

What is Aubaf Principle?

A

States that electrons are filled into atomic orbitals in the increasing order of orbital energy level.

70
Q

How many electrons can each orbital hold?

A

Two electrons

71
Q

What are metal/ non-metals near the divide with in between properties called?

A

Semi-metals or metalloids

72
Q

Which group is the divide between metals and non-metals clearest?

A

Group 14 (4)

73
Q

Which metal is liquid at room temperature?

A

Mercury

74
Q

What is a positive ion called?

A

Cation

75
Q

What elements do metallic bonding?

A

Between metals and metals

76
Q

What is metallic bonding?

A

Metallic bonding is the strong electrostatic attraction between cations (positive ions) and delocalised electrons. The cations are fixed in position, maintaining the structure and shape of the metal. The delocalised elections are mobile and are able to move throughout the structure. Only the electrons move.

77
Q

A metal structure, billions of metals atoms are held together by metallic bonding in a _____ ________ _______.

A

Giant metallic lattice

78
Q

What properties do most metals have?

A
  • Strong metallic bonds -> attraction between positive ions and delocalised electrons.
  • High electrical conductivity -> in both solid and liquid state.
  • High melting and boiling points.
79
Q

What does melting point depend on in metallic bonds?

A

The strength of the metallic bonds that hold the atoms together in the giant metallic lattice

80
Q

For most metals, high temperatures are necessary to provide the large amount of energy needed to overcome the strong _____________ __________ between the _______ and _________.

A
  • Electrostatic attraction
  • Cations
  • Electrons
81
Q

Are metals soluble?

A

No - they don’t dissolve.

82
Q

Which type of bonding is between non-metals and non-metals?

A

Covalent bonding.

83
Q

In a solid state, covalently bonded molecules form what type of structure that is held together by what?

A
  • Simple molecular structure
  • Weak intermolecular forces
84
Q

Do molecules that form simple molecular lattices have high or low boiling/ melting points?

A

Low

85
Q

Non-metals like _____, ______ and _______ have very different lattice structures - whereby the billions of atoms are held together by a network of what?

A
  • Boron, carbon and silicon
  • Form a network of strong covalent bonds to form a giant covalent structure
86
Q

What structure does carbon in its diamond form, form?

A

Tetrahedral structure

87
Q

How many bonds can a carbon atom have?

A

4 bonds

A-Level Chemistry (22 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions