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Chemistry > The Periodic Table (Chapter 7 & 8) > Flashcards

The Periodic Table (Chapter 7 & 8) Flashcards

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1
Q

How were elements arranged in early 1800s?

A

By physical and chemical properties

And by atomic mass

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2
Q

What did john newlands do?

A

When elements arranged in mass order every 8th element was similar

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3
Q

What did mendeleev do?

A

He arranged all elements by atomic mass and left gaps

He predicted undiscovered elements

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4
Q

What did Henry Moseley do?

A

Create the modern periodic table

In increasing atomic number (proton number)

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5
Q

Which groups are in the S block?

A

1 & 2

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6
Q

Where is the D block?

A

Transition metals

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7
Q

Which groups are in the P block?

A

3, 4, 5, 6, 7, 8

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8
Q

Define first ionisation energy

A

The first ionisation energy is the energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms.

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9
Q

Is ionisation endo or exothermic?

A

Exothermic

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10
Q

Write the equation for 1st ionisation energy of oxygen

A

O (g) —> O+ (g) + e-

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11
Q

What are the three factors affecting ionisation energy?

A

Nuclear charge

Atomic radius

Shielding

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12
Q

What does a high ionisation energy mean?

A

Strong attraction between the electron and the nucleus, so more energy is needed to overcome attraction and remove the electron

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13
Q

Does ionisation energy increase down a group or decrease down a group?

A

Increase as shells increase (gets bigger) easier to remove outer electron

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14
Q

What happens to ionisation energy across a period and why?

A

As you move across a period the general trend is for ionisation energy to increase.

No. Of protons increases which pulls electrons closer to positive nucleus, making atomic radius smaller.

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15
Q

Why is there a drop in ionisation energy between group 2 and 3?

A

Outer electron in group 3 is a P orbital rather than a S orbital

P orbital has higher energy than S orbital so is found further from nucleus

P orbital has additional shielding provided by the S electrons

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16
Q

Why do ionisation energies decrease between group 5 and 6?

A

In group 5, the electron is being removed from a singly occupied orbital

In group 6 elements, the electron is being removed from an orbital containing two electrons

The repulsion between two electrons in an orbital means that electrons are easier to remove from shared orbitals

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17
Q

Write the equation for 2nd ionisation energy for oxygen

A

O+ (g) —> O2+ (g) + e-

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18
Q

What do big jumps in ionisation energy indicate?

A

Occurs when an electron is being removed from a shell closer to the nucleus

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19
Q

What are Diamond, Graphite and Graphene examples of?

A

Giant covalent lattices

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20
Q

Why can carbon atoms form giant covalent lattices?

A

As they can each form four strong covalent bonds

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21
Q

What are different forms of the same element (in same state) called?

A

Allotropes

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22
Q

Is diamond hard or malleable?

A

Very hard

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23
Q

What shape is diamond?

A

Tetrahedral

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24
Q

Does diamond have a high melting point?

A

Yes extremely high

Sublimes at over 3800K

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25
Is diamond a good thermal conductor?
Yes as vibrations travel easily through its stiff lattice
26
Can diamond conduct electricity?
No, all outer electrons held in localised bonds
27
Can diamond dissolve in any substance?
no
28
Is silicone similar to diamond?
Yes it forms a crystal lattice with four strong covalent bonds off each carbon atom.
29
Are there delocalised electrons in graphite? If so where are they?
Yes The fourth outer electron is delocalised between the sheets of hexagons
30
How are the sheets of hexagons in graphite bonded together?
By weak induced dipole-dipole forces
31
How many bonds does each carbon form in graphite?
3
32
Why does graphite feel slippy?
Weak forces between layers easily broken, so sheets can slide over each other
33
Can graphite conduct electricity?
Yes Delocalised electrons free to move
34
Is graphite dense?
No- less dense than diamond As layers are far apart
35
What is graphite usually used for?
Lightweight and strong sports equipment
36
Does graphite have a high MP?
Strong covalent bonds so high MP Sublimes at over 3900K
37
Is graphite soluble?
NO
38
What is graphene?
One layer of graphite (2D)
39
What are the three properties of graphene?
Delocalised electrons in graphene free to move— makes it best known ELECTRICAL CONDUCTOR Delocalised electrons strengthen covalent bonds between carbon atoms (makes it very STRONG) Transparent and very light
40
What is graphene used in? (3)
Touchscreens Aircraft technology High-speed electronics
41
Does graphene have a high boiling point?
Yes due to strong covalent bonds
42
Is graphene insoluble?
Yep
43
Where are the delocalised electrons in a metal atom?
The outermost shell are delocalised
44
Can delocalised electrons move?
Yes they move about the metal, leaving a positively charged metal cation
45
Define metallic bonding
Metal cations are electrostatic-ally attracted to the negative delocalised electrons. They form a lattice of closely packed cation in a sea of delocalised electrons.
46
How does the number of delocalised electrons affect melting point?
The more delocalised electrons there are, the stronger the bonding will be and therefore higher the melting point
47
Why are metals malleable?
No bonds holding specific ions together, so they can slide past each other
48
Are metals soluble?
Metals are insoluble, except in Liquid Metal’s because of the strength of metallic bonds
49
What does more atoms in a molecule mean? (Simple molecules)
Stronger induced dipole forces
50
How does boiling point change across a period?
Type of bonding changes across a period Increases across metals and then sharp decrease after transition metals (Think logically)
51
How does reactivity change down group 2 and why?
Increases Ionisation energy decreases—> Easier to loose electrons
52
What are group 2 metals also known as?
Alkaline earth metals
53
Group 2 metal + water —>
Hydroxides
54
Group 2 metal + oxygen (burn) —>
Oxides
55
Group 2 metal + dilute acid —>
Salt and hydrogen
56
What are both group 2 oxide and hydroxides?
Bases Most soluble in water, so are also alkalis
57
What is an alkali?
A base that is soluble in water
58
Group 2 oxides + water —>
Metal hydroxides, which dissolve Magnesium oxide = exception, it reacts slowly and hydroxide isnt very soluble
59
Can group 2 compounds neutralise acidity?
Yes
60
list 2 examples where group 2 metals neutralise acidity
Calcium hydroxide- agriculture Magnesium hydroxide & calcium carbonate- used in indigestion tablets as antacids
61
What is group 7 also known as?
The halogens
62
What colour is fluorine gas?
Pale yellow
63
What colours is chlorine gas?
Greeeen
64
What colour is bromine liquid?
Red-brown
65
What colour is iodine solid?
Grey
66
Are the halogens diatomic?
Yes (two atoms joined by a single covalent bond)
67
Do the boiling points of halogens increase down or up the group?
Increase down the group
68
Why do the boiling points of the halogens increase down the group?
Increasing strength of London forces (induced dipole dipole) forces as the size and mass of the atoms increases
69
Does volatility increase or decrease down the halogens?
Decreases— physical state chlorine gas —> iodine solid
70
What is the trend in reactivity down the halogens?
Less reactive down the group
71
Why does reactivity decrease down the halogens?
Halogens need to gain an electron Going down the group atomic radii increase so outer electrons further away, this increases shielding which therefore decreases the attraction from the positive nucleus. Therefore harder to gain an electron.
72
Another way of saying the halogens get less reactive down the group?
Become less oxidising
73
Can halogens displace less reactive halide ions from solution?
Yes-
74
What is the colour of the organic layer: (in displacement reaction) Cl2 + Br- ?
Orange
75
What is the colour of the organic layer: (displacement reaction) Cl2 + I- ?
Violet
76
What is the colour of the organic layer: (displacement reaction) Br2 + I-
Violet
77
What is the test for halides?
Acidified Silver nitrate
78
What colour precipitate is formed: Chloride- Silver nitrate
White- dissolves in dilute & conc NH3 (aq)
79
What colour is the precipitate: Bromide- silver nitrate
Cream- dissolves in conc NH3 (aq)
80
What colour is the precipitate: Iodide- silver nitrate
Yellow- insoluble in conc & dilute NH3 (aq)
81
What is disproportionate reaction?
Which a single substance is both oxidised and reduced
82
Can halogens undergo disproportionation reactions?
Yes, with alkalis
83
Can the halogens exist as a wide range of oxidation states?
Yes Except fluorine
84
What makes bleach?
Chlorine and sodium hydroxide (Sodium chlorite (I) solution)
85
What is used to kill bacteria in water?
Chlorine- when mixed with water it undergoes disproportionation End up with hydrochloric acid and chloric (I) acid (CHLORATE IONS KILL BACTERIA)
86
Why is clean drinking water important?
Prevents water bound diseases (which 3.4 million people die of each year) ie. Cholera
87
What does the use of chorine in water treatment do? (3)
Kills disease causing microorganisms Some chlorine remains in water and prevents re-infection Prevents growth of algae, eliminating bad smell, taste and discolouration causes by organic compounds
88
What are the risks of using chlorine to treat water?
Chlorine gas is harmful- can irritate respiratory system Liquid chlorine can cause chemical burns Chlorine can react with organic compounds to form chlorinated hydrocarbons (some carcinogenic, but risk for cancer= small)
89
List 2 alternatives to using chlorine to treat water?
Ozone Ultraviolet Light
90
What is the test for carbonates?
Carbonate added to HCl- bubble the gas produced through limewater Carbon dioxide turns limewater cloudy
91
What is the test for sulfates?
Add dilute HCl, followed by barium chloride solution If white ppt produced, it will be barium sulfate (positive test)
92
Test for ammonium compounds?
Ammonia + sodium hydroxide —> warm it Any gas given off (if ammonia) will turn damp red litmus paper blue
93
How to remove false positives
Test in this order: Test for carbonates —> test for sulfates —> Test for halides

Chemistry (12 decks)

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