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Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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0
Q

Empirical Formula

A

Find masses
Look up give Ar values
Divide masses by Ar
Find ratio

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1
Q

Avogadro’s Number

A

6.022 x 10^23

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2
Q

% Element

A

ram x no of atoms / maximum mass of product x100

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3
Q

Rate of Reaction

A

product formed / time taken

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4
Q

Relative Mass and Charge

A

proton: 1 +1
neutron: 1 0
electron: 0 -1

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5
Q

Moles of Solute in a Solution

A

moles= concentration x volume

mol dm-3 = mol/dm3

dm-3 = 1000cm3

concentration: mol dm-3
volume: cm3

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6
Q

Moles in a Gas

A

moles= volume/24

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7
Q

Shapes of Molecules

A 
Electron pairs repel
Lone pairs repel more
bonding pairs
lone pairs
name
angle
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8
Q

Oxidation

A

The loss of electrons

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9
Q

Reduction

A

Gain of electrons

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10
Q

Oxidation Number

A

If it was ion, the charge is the same as the oxidation number.

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11
Q

Acids

A 
Release H+ ions in aqueous solution
Proton donor 
HCl hydrochloric
H2SO4 sulfuric
HNO3 nitric
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12
Q

Base

A

Neutralise acids
Proton acceptor
Soluble base that releases OH- ions in aqueous solution

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13
Q

Salt

A

A salt is formed when the H+ ion of an acid is replaced by a metal ion or ammonium ion

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14
Q

Neutralisation reaction

A

Acid + base –> salt + water

Acid + carbonate –> salt + water + CO2

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15
Q

Water of Crystalisation

A

Water molecules that form an essential part of the crystalline structure of a compound

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16
Q

Water of Crystallisation Moles

A

Calculate amount in moles of anhydrous
Then moles of water
Ratio to determine formula

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17
Q

Sub Shells

A

S- 2 electrons
P- 6 electrons
D- 10 electrons
F- 14 electrons

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18
Q

Orbitals

A

1- 1s
2- 2s, 2p
3- 3s, 3p, 3d
4- 4s, 4p, 4d, 4f

19
Q

Orbital filling order

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p

20
Q

Electronegativity Factors Effecting

A

Increases across the period- more protons and smaller radius

Decreases down the group- larger distance and more shielding

21
Q

Ionic bonding

A

Metals lose electrons +

Non metals gains electrons -

22
Q

Factors Effecting Metallic Bonding

A

Number of protons
Number of delocalised electrons
Size of ion

23
Q

Properties of metals

A 
Shiny 
Hard
Tough
Strong
Conductor of heat
Conductor of electricity 
High melting and boiling points
24
Q

Polar Intermolecular Bonds

A

has poles
hydrogen bonding
dipole-dipole

25
Q

Non Polar Intermolecular Bonds

A

Doesn’t have poles

Van der Waals

26
Q

Hydrogen Bonding

A

H-O
H-F
H-N

27
Q

Factors Affecting Ionisation Energy

A

Shielding
Nuclear charge
Radius size

28
Q

Advantages and Disadvantages of Chlorine

A
  • kills bacteria in water

- is toxic

29
Q

Salt

A

Compound formed when the hydrogen in an acid molecule is replaced by a metal ion or ammonium.

30
Q

Acid

A

A proton donor

31
Q

Base

A

A proton acceptor

32
Q

Group 2 Reactivity

A

Increases down the group

33
Q

Group 2 Reactions with Water

A

forms a metal hydroxide and hydrogen

Ca + 2H2O –> Ca(OH)2 + H2

34
Q

Group 2 Reactions with Oxygen

A

when burnt in oxygen, solid white oxides are produced

2Ca + O2 –> 2CaO

35
Q

Group 2 Oxides with Water

A

form metal hydroxides

CaO + H2O –> Ca2+ + 2OH-

product dissolves

36
Q

Group 2 Thermal Decomposition

A

CaCO3 –> CaO + CO2

37
Q

Group 2 Compound’s Uses

A

Ca(OH)2 calcium hydroxide, neutralises acid soils.

Mg(OH)2 magnesium hydroxide, indigestion tablets, neutralises excess stomach acids.

38
Q

What do acids do when mixed with water?

A

Release hydrogen ions

39
Q

Sulfuric acids produce salts called?

A

Sulfates

40
Q

Hydrochloric acids produce salts called?

A

Chlorides

41
Q

Nitric acids produce salts called?

A

Nitrates

42
Q

What happens when an acid reacts with a base?

A

They neutralise each other

acid + base –> salt + water

43
Q

What happens when an acid reacts with a metal?

A

metal + acid –> metal salt + hydrogen

44
Q

What happens when an acids reacts with a carbonate?

A

Metal carbonate + acid –> carbon dioxide + water

45
Q

how do van der waals forces arise?

A
  • uneven distribution of electrons
  • creates an instantaneous dipole
  • causes induced dipole in neighbouring molecules

Chemistry (6 decks)

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