Unit 1 Flashcards

(46 cards)

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
Polar Intermolecular Bonds
has poles hydrogen bonding dipole-dipole
25
Non Polar Intermolecular Bonds
Doesn't have poles | Van der Waals
26
Hydrogen Bonding
H-O H-F H-N
27
Factors Affecting Ionisation Energy
Shielding Nuclear charge Radius size
28
Advantages and Disadvantages of Chlorine
- kills bacteria in water | - is toxic
29
Salt
Compound formed when the hydrogen in an acid molecule is replaced by a metal ion or ammonium.
30
Acid
A proton donor
31
Base
A proton acceptor
32
Group 2 Reactivity
Increases down the group
33
Group 2 Reactions with Water
forms a metal hydroxide and hydrogen Ca + 2H2O --> Ca(OH)2 + H2
34
Group 2 Reactions with Oxygen
when burnt in oxygen, solid white oxides are produced 2Ca + O2 --> 2CaO
35
Group 2 Oxides with Water
form metal hydroxides CaO + H2O --> Ca2+ + 2OH- product dissolves
36
Group 2 Thermal Decomposition
CaCO3 --> CaO + CO2
37
Group 2 Compound's Uses
Ca(OH)2 calcium hydroxide, neutralises acid soils. Mg(OH)2 magnesium hydroxide, indigestion tablets, neutralises excess stomach acids.
38
What do acids do when mixed with water?
Release hydrogen ions
39
Sulfuric acids produce salts called?
Sulfates
40
Hydrochloric acids produce salts called?
Chlorides
41
Nitric acids produce salts called?
Nitrates
42
What happens when an acid reacts with a base?
They neutralise each other acid + base --> salt + water
43
What happens when an acid reacts with a metal?
metal + acid --> metal salt + hydrogen
44
What happens when an acids reacts with a carbonate?
Metal carbonate + acid --> carbon dioxide + water
45
how do van der waals forces arise?
- uneven distribution of electrons - creates an instantaneous dipole - causes induced dipole in neighbouring molecules