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Chemistry unit 1 > Chemistry Model Answers > Flashcards

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
SF6⃣
6 bond pairs BRE Octahedral 90
26
How are van der waal formed?
Uneven distribution if electrons Increase temporary dipole Induces dipole on neighbouring molecules
27
H2⃣O
``` 2 bond pair 1 lone pair LPRMTBP Angular or bent shape 104.5 ```
28
Simple molecular ( covalent ) structures
Any other covalent compound like H2⃣O, CH4⃣, Cl2⃣, CiCl4⃣ | All have intermolecular forces
29
Requirements for coordinate bonding
Lone pair of electrons | Space to accept pair of electrons
30
What different about graphite to the other giant covalent lattice molecules?
Intermolecular forces and some different properties
31
Comparison between properties of graphite and the other covalent structures
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
H----Cl Polar or non polar? Explain
Polar Non symmetrical Dipole do not cancel Permanent dipole
33
Explain why S8⃣ has a higher melting point the Cl2⃣
S had stronger van der waal forces than Cl | S has more electrons in its structure
34
CCl4⃣ Polar or non polar? Explain
Non polar Symmetrical Dipoles cancel Van der waals
35
BF3⃣ | Bonding and structure?
3 bind pairs BRE Trigonal planar 120
36
Unusual facts about water
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
H2⃣O Polar or non polar? Explain
Polar Non symmetrical Dipoles do not cancel Permanent dipole
38
Explain why the electrical conductivity increases from Na to Al
Number of delocalised electrons in metallic lattice increase
39
Explain why the elements P to Ar cannot conduct electricity
They contain no delocalised electrons or mobile ions
40
Group two reactions with water
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
Explain why the melting and boiling point increase from Na to Al
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
Explain why silicon has such a high melting point
Silicon has a giant covalent structure Contain many string covalent bonds Large amount of heat energy needed to break the bonds
43
Melting points down group two elements
``` 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
Reaction with oxygen - group two
Group two metals react more vigorously down the group when reacted with group 2
45
Properties of intermolecular forces
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
What colour is bromine at rtp and state?
Red brown liquid
47
Group 2 reaction with oxides
More soluble down the group Down the group gets more basic No redox reactions
48
Group 2 carbonates
Thermal decomposition increases down the group No effervescence Down group carbonates are more difficult to decompose
49
What colour is fluorine at rtp and state?
Yellow gas
50
Boiling point down group 7
Increases More electrons More van der waals More energy needed to break bonds
51
What colour is chlorine at rtp and state?
Green gas
52
What colour is iodine at rtp and state?
Grey solid
53
Electro negativity down group 7
``` Decreases Nc increases outweighed by shielding NA decrease AR increase Shielding increase ```
54
Ionic equation when mixing silver nitrate
Ag+ (aq) + Cl- (aq) ----> AgCl (s)
55
Reactivity down group 7
``` Decreases AR increase Shielding increase NC increase is outweighed NA decrease Elements find harder to gain electrons ```
56
Are halogens good oxidising agents?
Yes
57
What is the reactivity down group two
``` Increases Atomic radii increase Shielding increase Nuclear charge increase but outweighed by shielding Nuclear attraction decrease Outer electron lost more easily ```
58
Colours of halogens in organic solvents like cyclohexane A) chlorine B) bromine C) iodine
A) pale green B) orange C) purple/lilac
59
Chlorine with water symbol and word equation | What sort of reaction is this?
Cl2⃣ (g) + H2⃣O (l) --> HCl (aq) + HClO (aq) Chlorine plus water gives hydrochloric acid plus chloric (I) acid. Disproportionation reaction
60
In the reaction with chlorine and water, why is chlorine used? What is wrong with using chlorine?
Chlorate ion kills bacteria | Chlorine is toxic
61
What does chlorine and cold, aqueous sodium hydroxide make?
Bleach
62
Solubility of halides in dilute ammonia solution A) chloride B) bromide C) iodide
A) soluble B) insoluble C) insoluble
63
Colours of Halogens in aqueous solution : A) chlorine B) bromine C) iodine
A) pale green B) orange C) brown
64
Solubility of halides in concentrated ammonia solution A) chloride B) bromide C) iodide
A) soluble B) soluble C) insoluble
65
Test for halides
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

Chemistry unit 1 (12 decks)

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