Chemistry Flashcards

1
Q

Structure of an atom

A

An atom has a central nucleus. This is surrounded by electrons arranged in shells.

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2
Q

Electron

A

Negative charge and very small

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3
Q

Proton

A

Positive charge and same size as neutron

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4
Q

Neutron

A

Neural charge and same size as proton

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5
Q

Where is the majority of mass of an atom located?

A

Nucleus

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6
Q

Atomic Number

A

The number of protons (smaller number)

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7
Q

Mass number

A

The number of protons and neutrons (bigger number)

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8
Q

Isotope

A

Same number of protons and electrons but different number of neutrons

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9
Q

Concept of relative atomic mass

A

Weighted mean of masses of the atoms of isotopes.

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10
Q

Calculating Ar

A

Total mass of atoms/Total percentage

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11
Q

Where are periods?

A

Horizontal rows

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12
Q

Where are groups?

A

Vertical columns

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13
Q

How are elements ordered?

A

In order of increasing atomic number

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14
Q

Group 1

A

Alkali metals

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15
Q

Group 2

A

Alkaline earth metals

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16
Q

Group 16

A

Common non-metals

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17
Q

Group 17

A

Halogens

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18
Q

Group 18

A

Noble gases

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19
Q

Transition metal properties

A

Conduct electricity in solid and liquid states

Shiny when freshly cut

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20
Q

Transition metals compared to group 1 metals

A

Higher melting points
Higher density
Greater strength
Greater hardness

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21
Q

Electron configuration

A

Atomic number (protons)

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22
Q

What happens down a metal group?

A

Reactivity increases

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23
Q

What happens down a non-metal group?

A

Reactivity decreases

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24
Q

What do elements in the same group have in common?

A

Similar chemical properties

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25
Can the nuclei be created or destroyed?
No
26
State symbol (S)
Solid
27
State symbol (L)
Liquid
28
State symbol (G)
Gas
29
State symbol (AQ)
Aqueous solution
30
What is an equilibrium?
A situation where forward and back reactions happen at the same rate, and the concentration of substances stay the same.
31
Factors that affect equilibrium
Concentration of reactants/products Temperature Overall pressure
32
How do you use Ar to work out Mr? Use CO2 as an example
Example CO2: Ar of C = 12 | Ar of O = 16 12+16+16 = 44 Mr of CO2 = 44
33
What is Avogadro’s number?
The number of particles in one mole of a substance
34
What value is Avogadro’s constant?
6.02 x 10^23
35
What is one mole of a substance?
Ar or Mr in grams
36
How to work out percentage composition?
Total Ar of element/Mr of compound | x100
37
What is empirical formula?
Simplest integer ratio of atoms
38
Conditions for ideal gas
One mole of gas occupies a set volume at a given temperature or pressure. (24dm^3)
39
What is concentration measured in?
mol dm ^-3 or g dm^-3
40
Saturated Solution
A solution that contains the maximum amount of solute taht is capable of being dissolved.
41
Titration calulations
Watch youtube video
42
Percentage yield
``` Actual yield(g)/Predicted yield(g) X100 ```
43
Oxidation
Gain of oxygen
44
Reduction
Removal of oxygen
45
Oxidation in terms of electron
Gain of electrons
46
Reduction in terms of electron
Removal of electrons
47
How to identify oxidation only?
//
48
How to identify reduction only?
//
49
How to identify a redox (both oxidation and reduction) ?
//
50
How to identify a non-oxidation/reduction?
//
51
Oxidising agent
Normally non-metal or positive ion
52
Reducing agent
Normally metal or negative ion
53
Element
A substance that only has one type of atom and it cannot be broken down into anything simpler
54
Compound
A substance made up of 2 or more elements chemically bonded
55
Mixture
Consists of 2 or more substances, not chemically bonded
56
What do atoms often react to form?
Compounds that have an election configuration of a noble gas (group 18)
57
Ionic bonding
Metals and non-metals reacting leading to electrons going from metals to non-metals.
58
Anion
Gains electrons and becomes negatively charged
59
Cation
Loses electrons and becomes positively charged
60
NH4+
Ammonium
61
Ca2+
Calcium
62
Na+
Sodium
63
Pb2+
Lead
64
OH-
Hydroxide
65
NO3-
Nitrate
66
CO3^2-
Carbonate
67
SO4^2-
Sulfate
68
What do roman numerals after an element suggest?
When an element has more than 1 oxidation state, the roman numerals denote which is present e.g. iron (lll)
69
Physical properties of Ionic compounds
High boiling and melting points Solid at room temp Cannot conduct electricity in solid state Can conduct in molten or in solution state Strong electrostatic forces Hard and brittle
70
Covalent bonding
Bonding between 2 non-metals (sharing of electrons)
71
Covalent molecules can be...
Small molecules or giant structures
72
Small covalent molecules
Water (H20) Ammonia (NH3) Methane (CH4)
73
Giant covalent structures
Diamond (C) Graphite (C) Silicon dioxide (SiO2)
74
Physical properties of small covalent molecules
Low melting and boiling points Does not conduct electricity (Strong covalent bonds, weak intermolecular forces)
75
Physical properties of giant covalent properties
Very high melting points | Variable electricity conductivity (Diamond doesn't, graphite does and silicon is midway)
76
Metallic bonding
The strong electrostatic force of attraction between metal ions
77
What do solid metals exist as?
Solid metals exist as a giant structure of positively charged ions surrounded by delocalised electrons.
78
Physical properties of metals
``` Shiny High melting and boiling points Good conductor of heat and electricity High density Malleable and ductile ```
79
Where are intermolecular forces and how do you overcome them?
They exist between molecules and must be overcome in melting and boiling.
80
Physical and chemical properties of alkali metals (group 1)
Physical - soft (can be cut with a knife) and low melting points Chemical -