Unit 2 Flashcards

Periodic Table (30 cards)

1
Q

What does the property of an element depend on?

A

Atomic number (protons)

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2
Q

How is the periodic table arranged?

A

In atomic numbers

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3
Q

How many electrons does each orbital hold?

S P D F

A

2
6
10
14

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4
Q

What does a period tell you?

A

Energy level. (number of shells)

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5
Q

What does group tell you?

A

Number of valence electrons

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6
Q

Trends in atomic radius

A

↓← Decrease across a period is due to more protons meaning more attraction
Increase down a group is due to shielding

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7
Q

What is ionisation energy?

A

Amount of energy needed to remove an electron from an atom in gas phase

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8
Q

Trend in ionisation energy?

A

↑→ increases across a period as more protons and no increased shielding.
Decreases down a group as shielding increases

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9
Q

What is metallic character?

A

How readily an atom can lose an electron. So highly electronegative elements (eg) fluorine have very little metallic character

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10
Q

Trend in metallic character?

A

↓← (opposite of ionisation) more shielding less attraction to the nucleus

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11
Q

Properties of metals?

A
Good electric and heat conductors.
Malleable 
Solid at room temp
Lose valence shells easily 
Reducing agent
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12
Q

Non metal properties

A
Poor electric and heat conductors 
brittle
many forms at room temp
Gain valence shells 
Oxidizing agent
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13
Q

what is a hydride?

A

Compound formed by hydrogen and another element only

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14
Q

What are covalent hydrides?

A

H+ Non- metal

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15
Q

What are ionic hydrides?

A

H+ metal

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16
Q

What are metallic hydrides?

A

h+ transition metal

17
Q

What is an oxide?

A

An oxygen and another element only

18
Q

What are acidic oxides?

A

Oxides of non metals. Also known as acid anhydrides

19
Q

What are basic oxides?

A

Oxides of group 1 and 2 aka base anhydrides

20
Q

What is an amphoteric solution?

A

Can act as both an acid or a base

21
Q

What is an amphoteric oxide?

A

A metallic oxide that shows both acidic and basic properties

22
Q

What is a diagonal relationship?

A

The fact that metallic character increases down a group and decreases across a period means they cancel out diagonally. Meaning diagonal elements can have similar properties.

23
Q

What element has the highest ionisation energy?

A

Helium. i.E increases up a group and across a period

24
Q

Is high electronegativity a characteristic of metals or non metals?

25
Is oxidising ability a property of metals or non metals
Non metals
26
is being a poor electrical conductor a property of metals or non metals?
Non metals
27
Is being opaque when thin a characteristic of metals or non metals?
Metals
28
Are ionic hydrides soluble?
No
29
What are metallic hydrides also known as?
Interstitial hydrides
30
Explain the trend in boiling points
looking at periods 2 and 3 the boiling point increases until C and si . This is because they have giant metallic structures. and the nuclear charge is getting bigger so increased attraction meaning harder to separate them. C and Si are giant covalently bonded so have even higher. Melting points drop and N and P b/c simple covalent bonds aren't as strong, so don't need as much energy. Mr also affects these, heavier means more van der waals