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Chemistry Year 1 AS > EL 8 Spectacular Metals > Flashcards

EL 8 Spectacular Metals Flashcards

1
Q

Physical Properties of Metals (9)

A
  • Malleable
  • Sonorous
  • High Density
  • Shiny
  • Ductile
  • Good Thermal Conductor
  • Good Electrical Conductor
  • High Melting Point
  • High Boiling Point
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2
Q

Explain bonding in metals [3 marks]

A
  • Metallic Bonding
  • The outer electrons of metals become delocalised and are free to move in a sea of electrons
  • Positively charged metallic cations are attracted to the delocalised negatively charged electrons
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3
Q

Group 1 and 2 Metal Properties (3)

A
  • Soft = Easy to cut
  • Weak = Breaks easily
  • Low melting point
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4
Q

Group 1 and 2 Metal Origins (What are they found as)

A
  • Highly reactive = Found as cations (Positively charged ions)
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5
Q

Define “salt”

A

A chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions

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6
Q

Group 1 and 2 Metals react with water to form…?

A

Metal + Water —> Metal Hydroxide and Hydrogen

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7
Q

Group 1 Metals are known as…?

A

Alkaline Metals

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8
Q

Group 2 Metals are known as…?

A

Alkaline Earth Metals

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9
Q

Hydroxide Ion

A

OH 1-

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10
Q

Nitrate Ion

A

NO3 1-

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11
Q

Sulphate Ion

A

SO4 2-

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12
Q

Carbonate Ion

A

CO3 2-

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13
Q

Hydrogen Carbonate Ion

A

HCO3 1-

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14
Q

Group 1 and 2 Metals react with oxygen to form…?

A

Metal + Oxygen —> Metal Oxide

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15
Q

Group 1 and 2 Metals react with halogens to form…?

A

Metal + Halogen —> Metal Halide

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16
Q

Why are Group 1 and 2 Metals more reactive as you go down? (3)

A

i) Greater Number of Shells

ii) Electron Shielding

iii) Greater Nuclear Charge

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17
Q

Why are Group 1 Metals more reactive than Group 2 Metals?

A

Group 1 = 1 electron to be removed

Group 2 = 2 electrons to be removed

Therefore, Group 2 requires more energy = less reactive

18
Q

Group 2 Metal Oxides react with water to form…?

A

Metal Oxide + Water —> Metal Hydroxide

19
Q

Group 2 Metal Oxides react with acid to form…?

A

Metal Oxide + Acid —> Salt + Water

20
Q

Group 2 Metal Hydroxides react with acid to form…?

A

Metal Hydroxide + Acid —> Salt + Water

21
Q

Group 2 Metal Hydroxides dissolve in water to form…?

A

Metal Hydroxide —-> Metal Ions + Hydroxide Ions

22
Q

Factors affecting Charge Density (2)

A
  • Ions with a smaller radius = higher charge density
    —> i.e. found at the top of groups in the periodic table
  • Ions with a greater charge = higher charge density
    —> Al3+ > K+
23
Q

Group 2 Carbonates Thermal Stability Trend

A

As you go down Group 2, thermal stability increases (requires more heat) since there is less distortion

24
Q

Group 2 Hydroxides Solubility Trend

A

As you go down Group 2, solubility increases

25
Q

Group 2 Sulphates & Carbonates Solubility Trend

A

As you go down Group 2, solubility decreases

26
Q

Define First Ionisation Enthalpy

A

The energy requires to remove one electron from every atom in one mole of isolated gaseous atoms

27
Q

First Ionisation Enthalpy Equation

A

X(g) —> X+(g) + e-

28
Q

Shape of a s subshell

29
Q

Number of orbitals in a s subshell

A

One Orbital

30
Q

Shape of a p subshell

31
Q

Number of orbitals in a p subshell

A

Three Orbitals

32
Q

Shape of a d subshell

A

Double Dummbell

33
Q

Number of orbitals in a d subshell

A

Five Orbitals

34
Q

How many electrons can fit in a single orbital?

35
Q

Factors which affect Ionisation Enthalpy (3)

A

i) Atomic Radius
Larger radius = Less energy required

ii) Electron Shielding
More shields lead to more shielding = Less energy required

iii) Nuclear Charge
The number of protons in the nucleus influences the Ionisation Energy

36
Q

Why is there a drop in Ionisation Energy between Group 2 and 3?

A

The addition of a p subshell

37
Q

Why is there a drop in Ionisation Energy between Group 5 and 6?

A

The electron repulsion when the 4th electron occupies its position in the orbital

38
Q

Thermal Decomposition of a Metal Carbonate

A

MCO3(s) —> MO(s) + CO2(g)

39
Q

Group 2 Hydroxide’s pH in Water Trend

A

As you go down Group 2, pH increases

40
Q

As you go across a Period, what happens to the Ionisation Energy and why is this?

A

Number of Shells and Shields stay the same = These factors have no effect on the Ionisation Energy

Nuclear Charge Increases = Ionisation Energy generally increases

41
Q

Example : Why is AlCl3 more distorted than NaCl?

A

The cation Al 3+ has a greater charge than that of the cation Na +, therefore Al 3+ has a higher charge density than Na +

42
Q

Example : Why is AlF3 less distorted than AlBr3?

A

The anion F- has a smaller radius than that of the anion Br-, therefore Br- has a lower charge density and is more readily distorted

Chemistry Year 1 AS (9 decks)

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