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Chemistry Model Answers Flashcards

1
Q

Hydroxide and acid makes…

A

Salt

Water

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2
Q

BF5⃣

A

5 bond pairs
BRE
Trigonometry bipyramidal
120 or 90

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3
Q

Ammonia and acid makes…

A

Ammonium salt NH4⃣

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4
Q

Acid and alkali makes?

A

Salt

Water

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5
Q

Acid and metal carbonate makes…

A

Salt
Water
Carbon dioxide

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6
Q

Oxide and acid makes

A

Salt

Water

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7
Q

Ionisation energy down a group

A 
Decreases because ...
NC increases but outweighed shielding
AR increase
NA decrease 
Shielding increase
Easier to remove outmost electron
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8
Q

Common acids

A

HCl
H2⃣SO4⃣
HNO3⃣

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9
Q

Hydrocarbonates and acid makes..

A

Salt
Water
Carbon dioxide

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10
Q

Writing ionic equation

A

Only separate aqueous solutions

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11
Q

Observations

A

Dissolving of metals, metal carbonates or soluble bases when reacted with acid

Effervescence is gas is produced

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12
Q

Common bases

A

Metal oxides
Metal hydroxides
Ammonia

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13
Q

Properties of giant metallic lattices

A 
High melting points
Strong due to attractions between ions and delocalised electrons
Malleable 
Ductile
Not brittle 
They conduct - delocalised electrons
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14
Q

NH3⃣

A 
3 bond pairs
1 lone pair
LPRMTBP
Pyramidal
107
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15
Q

Command alkalise

A

Sodium hydroxides
Potassium hydroxide
Aqueous ammonia

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16
Q

Ionisation energy across a period…

A 
Increases because...
NC increase
AR decrease
NA increase
Shielding insignificant
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17
Q

Why is helium the highest first ionisation energy?

A

Electrons occupy the first shell
Electrons are very close to the nucleus
No other electrons so no shielding
More protons than hydrogen so stronger nuclear charge so electrons are held more strongly

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18
Q

Van der waal going down the group

A

More electrons
More van der waals
More energy needed to break them

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19
Q

Drawing an ionic bond

A

Anions have a mixture of its own and transferred electrons
Cations have no electrons shown
Relevant charges on the outside of the squared brackets

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20
Q

What does an acid and metal make?

A

Salt

Hydrogen

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21
Q

Giant ionic lattice properties and explanations

A

High melting and boiling point - held together by string ionic bonds in the lattice so a lot of energy is needed to break the bonds

Very brittle - if the layers slide over each other, the charges with repel each other

Do not conduct when solid - ions are held strongly in lattice

Conduct when molten or aqueous - ions are mobile

Insoluble in non polar solvents - soluble in water because it is polar

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22
Q

BeCl2⃣

Describe bonding and structure

A

2 bond pairs
Bonds pair repel equally
Linear
Bind angle is 180

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23
Q

Giant covalent lattice examples

A

Diamond
Graphite
Silicon
Silicon dioxide

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24
Q

CH 4⃣

Bonding and structure

A

4 bond pairs
BRE
Tetrahedral
109.5

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25
Q

SF6⃣

A

6 bond pairs
BRE
Octahedral
90

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26
Q

How are van der waal formed?

A

Uneven distribution if electrons
Increase temporary dipole
Induces dipole on neighbouring molecules

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27
Q

H2⃣O

A 
2 bond pair
1 lone pair
LPRMTBP
Angular or bent shape
104.5
28
Q

Simple molecular ( covalent ) structures

A

Any other covalent compound like H2⃣O, CH4⃣, Cl2⃣, CiCl4⃣

All have intermolecular forces

29
Q

Requirements for coordinate bonding

A

Lone pair of electrons

Space to accept pair of electrons

30
Q

What different about graphite to the other giant covalent lattice molecules?

A

Intermolecular forces and some different properties

31
Q

Comparison between properties of graphite and the other covalent structures

A

Diamond, silicon and silicon dioxide
High melting points due to strong covalent bonds therefore large amount of energy required
Hard as they exist in a rigid tetrahedral structure with coordination number if 4
Does not conduct because there are no mobile electrons as the carbon use all four atoms for bonding

Graphite
High melting points due to strong covalent bonds therefore large amount of energy required
Soft because it consists of layers attracted by weak van der waal forces and layers slide over each other
Conducts electricity because each atom only uses 3 of its outer shell electrons for bonding ( coordination number of 3) and remaining delocalised electrons can move through layers allowing conductivity

32
Q

H—-Cl
Polar or non polar?
Explain

A

Polar
Non symmetrical
Dipole do not cancel
Permanent dipole

33
Q

Explain why S8⃣ has a higher melting point the Cl2⃣

A

S had stronger van der waal forces than Cl

S has more electrons in its structure

34
Q

CCl4⃣
Polar or non polar?
Explain

A

Non polar
Symmetrical
Dipoles cancel
Van der waals

35
Q

BF3⃣

Bonding and structure?

A

3 bind pairs
BRE
Trigonal planar
120

36
Q

Unusual facts about water

A

Ice - simple molecular lattice, volume larger than the water making it, ice floats due to hydrogen bonds being further apart

Water has higher than expected boiling point - hydrogen bond is strongest intermolecular force
Water expands when frozen therefore ice is less dense - hydrogen bonds are longer than covalent so takes up greater volume
High surface tension due to extra attraction between molecule just below the surface
High viscosity of water

37
Q

H2⃣O
Polar or non polar?
Explain

A

Polar
Non symmetrical
Dipoles do not cancel
Permanent dipole

38
Q

Explain why the electrical conductivity increases from Na to Al

A

Number of delocalised electrons in metallic lattice increase

39
Q

Explain why the elements P to Ar cannot conduct electricity

A

They contain no delocalised electrons or mobile ions

40
Q

Group two reactions with water

A

Mg + 2H2⃣O —> Mg(OH)2⃣ + H2⃣
Works for any metal down group 2

Mg + 2H2⃣O –(steam)–> MgO + H2⃣
Only magnesium

Mg(OH)2⃣ pH 8. Used in antacids or toothpaste. |
Ca(OH)2⃣ pH 10. Used to neutralise acidic soil. |
Sr(OH)2⃣ pH 12. |
Ba(OH)2⃣ pH 14. |
¥
Hydroxide more soluble down a group

Group two metals react more vigorously with cold water

41
Q

Explain why the melting and boiling point increase from Na to Al

A

Strength of metallic bond increases
Number of delocalised electrons added to metal structure increases
Al has a greater charge of +3
Therefore more energy is needed to break the bonds

42
Q

Explain why silicon has such a high melting point

A

Silicon has a giant covalent structure
Contain many string covalent bonds
Large amount of heat energy needed to break the bonds

43
Q

Melting points down group two elements

A 
Decreases
Nuclear attraction decrease
Nuclear charge increases but outweighed by shielding
Shielding increases 
Easier to remove outermost electron
Weaker metallic bonds
Ionic radii increase
44
Q

Reaction with oxygen - group two

A

Group two metals react more vigorously down the group when reacted with group 2

45
Q

Properties of intermolecular forces

A

Low boiling point due to weak intermolecular van der waal forces so little energy is needed
As a result they tend to gases or liquid at room temperature
Iodine is an exception

Do not conduct electricity due to not mobile electrons

More soluble in organic solvents than water due to van der waal forces between molecular structure and solvent molecule

46
Q

What colour is bromine at rtp and state?

A

Red brown liquid

47
Q

Group 2 reaction with oxides

A

More soluble down the group
Down the group gets more basic
No redox reactions

48
Q

Group 2 carbonates

A

Thermal decomposition increases down the group
No effervescence
Down group carbonates are more difficult to decompose

49
Q

What colour is fluorine at rtp and state?

A

Yellow gas

50
Q

Boiling point down group 7

A

Increases
More electrons
More van der waals
More energy needed to break bonds

51
Q

What colour is chlorine at rtp and state?

A

Green gas

52
Q

What colour is iodine at rtp and state?

A

Grey solid

53
Q

Electro negativity down group 7

A 
Decreases 
Nc increases outweighed by shielding
NA decrease
AR increase
Shielding increase
54
Q

Ionic equation when mixing silver nitrate

A

Ag+ (aq) + Cl- (aq) —-> AgCl (s)

55
Q

Reactivity down group 7

A 
Decreases
AR increase
Shielding increase
NC increase is outweighed
NA decrease
Elements find harder to gain electrons
56
Q

Are halogens good oxidising agents?

A

Yes

57
Q

What is the reactivity down group two

A 
Increases 
Atomic radii increase
Shielding increase 
Nuclear charge increase but outweighed by shielding
Nuclear attraction decrease
Outer electron lost more easily
58
Q

Colours of halogens in organic solvents like cyclohexane
A) chlorine
B) bromine
C) iodine

A

A) pale green
B) orange
C) purple/lilac

59
Q

Chlorine with water symbol and word equation

What sort of reaction is this?

A

Cl2⃣ (g) + H2⃣O (l) –> HCl (aq) + HClO (aq)

Chlorine plus water gives hydrochloric acid plus chloric (I) acid.

Disproportionation reaction

60
Q

In the reaction with chlorine and water, why is chlorine used?
What is wrong with using chlorine?

A

Chlorate ion kills bacteria

Chlorine is toxic

61
Q

What does chlorine and cold, aqueous sodium hydroxide make?

A

Bleach

62
Q

Solubility of halides in dilute ammonia solution
A) chloride
B) bromide
C) iodide

A

A) soluble
B) insoluble
C) insoluble

63
Q

Colours of Halogens in aqueous solution :
A) chlorine
B) bromine
C) iodine

A

A) pale green
B) orange
C) brown

64
Q

Solubility of halides in concentrated ammonia solution
A) chloride
B) bromide
C) iodide

A

A) soluble
B) soluble
C) insoluble

65
Q

Test for halides

A

Add aqueous silver nitrate and if white precipitate forms chloride present

If cream precipitate forms bromide is present

If yellow precipitate forms iodide is present

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