EL8 Spectacular Metals Flashcards

1
Q

Define ionisation energy

A

Energy required to remove an electron from an atom, forming a positive ion

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2
Q

Define first ionisation energy

A

Energy required to remove 1 electron from each atom in 1 mole of gaseous atoms

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3
Q

How does atomic radius affect ionisation energy?

A
  • as atomic radius increases, I.E decreases, due to weaker nuclear attraction
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4
Q

How does nuclear charge affect ionisation energy?

A
  • greater the nuclear charge, greater nuclear attraction, I.E increases
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5
Q

How does electron shielding affect ionisation energy?

A
  • inner shells of electrons repel outer electrons, therefore more inner shell means greater shielding, less nuclear attraction therefore lower I.E
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6
Q

Why do successive ionisation energies increase?

A

As electrons are removed, nuclear charge increases, ionic radius decreases, nuclear attraction increases

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7
Q

How can a graph showing successive ionisation energies allow you to predict the group of an element?

A
  • there are large jumps between each energy level
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8
Q

Define electronegativity

A

Relative ability of atoms to attract electrons in a covalent bond

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9
Q

Does electronegativity increase or decrease across a period? And why

A
  • increases

- atomic radius decreases, stronger nuclear attraction

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10
Q

Does electronegativity increase or decrease down a group? And why

A

Decrease

- atomic radius increases, weaker nuclear attraction

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11
Q

What are group 1 elements known as?

A

Alkali metals

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12
Q

What are group 2 elements known as?

A

Alkali earth metals

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13
Q

Do elements in groups 1 and 2 become more or less metallic down group?

A
  • more metallic

- reactivity increases down group

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14
Q

Do elements become more or less metallic across a period?

A
  • less metallic

- reactivity decreases across period

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15
Q

What is formed when group 2 metals react with water?

A

Metal hydroxide and hydrogen

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16
Q

Give equation for reaction between calcium and water

A

Ca(s) + H20(l) Ca(OH)2(aq) + H2(g)

17
Q

What is calcium hydroxide used for?

A
  • neutralising acidic soil
18
Q

What is magnesium hydroxide used for?

A

Neutralising stomach acid

19
Q

What is produced when group 2 elements react with oxygen?

A

Group 2 oxides

20
Q

Give equation for magnesium and oxygen

A

2Mg(s) + O2(g) 2MgO(s)

21
Q

What happens when group 2 oxides are dissolved in water?

A

Aqueous solution of metal hydroxide is produced

22
Q

What is produced when group 2 carbonates undergo thermal decomposition?

A

Metal oxide and carbon dioxide

23
Q

Give equation of thermal decomposition of calcium carbonate

A

CaCO3(s) –> CaO(s) + CO2(g)

24
Q

Does thermal decomposition become easier or harder down group and why?

A
  • harder
  • smaller ions have greater charge density, therefore greater polarising effect on negatively charged cloud around carbonate ion, therefore carbonate is less stable