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Chemistry > Topic 1 - Key concepts in Chemistry > Flashcards

Topic 1 - Key concepts in Chemistry Flashcards

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1
Q

23
Na
11

what is the top number

A

The relative atomic mass

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2
Q

23
Na
11

what is the bottom number

A

the atomic number

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3
Q

What is the relative atomic mass?

A

The total number of protons and neutrons

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4
Q

What is the atomic number

A

The number of protons (therefore the number of electrons)

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4
Q

What are isotopes?

A

an element which can have different numbers of neutrons

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5
Q

Proton

A

Mass of 1
positive charge

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6
Q

electron

A

very small mass
negative charge

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7
Q

neutron

A

mass of 1
no charge

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8
Q

The equation for Relative atomic mass

A

(rm x ra) + another dpending on how many / total abundance

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9
Q

Electron configuration rules

A

The first shell can only contain 2 electrons
the shells after hold 8
fill from in to out

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10
Q

What do atoms think when they dont have a full outer shell?

A

They wanna be stable, so they want to chemically react.

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11
Q

what are bonds?

A

forces of attraction that holds the atoms together

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12
Q

what type of atom changes name when turning into ion? what ending?

A

Non- metals and ends with ide or ate

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13
Q

What is an ion?

A

an atom or group of atoms that have lost / gained electrons resulting in a net charge

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14
Q

What are cations

A

Metals will always loose electrons and become postively cvharged.

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15
Q

Wat are anions

A

A
Non metals will gain electrons and become negatively charg

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16
Q

Ionic bonding between

A

metal and non metal

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17
Q

Ionic Bonding vs Covalent Bonding

A

Covalent bonding between 2 non metals.
ionic is a metal and a non metal

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18
Q

What are ionic compounds

A

ionic compounds contain one or more cation paired with one or more anion
they are formed by the loss or gain of electrons
they are held together by strong electrostatic forces of attraction between opposely charges ions

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19
Q

Why do ions form lattice structures?

A

They are because the stong electrostatic forces let “billions” of ions to be packes together in this regular repeating structure

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20
Q

What does the ending ide or ate mean in a ion?

A

it shows the ion has oxygen and another element in it

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21
Q

Why do ionic compounds have such a high melting and boilig point?

A

there is strong electrostatic forces that hold them together, it takes alot of energy to break these bonds

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22
Q

When do ionic compounds conduct electricity?

A

WHen they are molten or dissolved in water
its the chargged ions that carry the current, so they need to be free to conduct

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23
Q

What 2 conditions must be met for a thing to conduct electricity?

A

It must contain charged particles
these particles must be free to move

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24
Q

What are simple molecular substances ?

A

molecules held together by covalent bonds

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25
Q

When are covalent bonds usually formed?

A

between 2 non metals sharing pairs of electrons

They are strong

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26
Q

How are the atoms in molecules held together?

A

the strong electrostatic forces of attraction between the nuclei and the shared electrons

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27
Q

how are ionic compounds electrically neutral?

A

the 2 components have balancing positive charge and negative charge

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28
Q

Why do ionic copounds only conduct when molten or in aqueous solution?

A

The particles to be free to carry the current for it is the charged ions that actually carry it.

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29
Q

What is the law of conservation of mass?

A

In a chemical reaction, mass is always conserved in a closed system

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30
Q

Concentration =

A

mass of solute in g/
volume of solution in dm3

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31
Q

Why may mass appear to be lost in an open system?

A

the products may be gases released into the air

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32
Q

What is the Empirical formula?

A

the simplest whole number ratio of atoms or ions of each element in a substence

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33
Q

As well as Empirical formula, what do simple molecules have?

A

A molecular formula

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34
Q

Molecular formula

A

the amount of atoms of each element actually in that molecule

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35
Q

What is the symbol for relative formula mass?

A

Mr

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36
Q

What is the symbol for relative atomic mass?

A

Ar

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37
Q

How do you calculate Mr

A

Add the Ars in the compound

38
Q

How to calculate Empirical formula

A

Mass / Mr
then divide by smallest number

39
Q

What is a Mole

A

an amount fo particles
1 mole = Mr or Ar of a molecule

40
Q

What is the formula triangle envolving mass, Mr and moles

A

Mass
Mr I Moles

41
Q

What is avogadro’s constant?

A

6.02 x 10^23

42
Q

How do you turn cm3 into dm3

A

/1000

43
Q

Diamond structure

A

4 Covalent bonds per atom
Forms tetrahedons

44
Q

Properties of diamond

A

very high melting and boiling points
Does not conduct electricity
Very hard
Insoluble in water

45
Q

Giant covalent structures properties

A

Strong covalent bonds between atoms
High melting and boiling points
usually poor conductors of electricity
usually solid at RT
Very poor solubility in water

46
Q

Allotrope

A

Different structural form of the same element

47
Q

Why does diamond have high melting and boiling points?

A

Strong covalent bonds take alot of energy to overcome

48
Q

Why is diamond hard?

A

It is resistant to scratching cutting or denting because it is bonded with 4 covalent bonda witha tetralhedral structure

Drill tips

49
Q

Why is diamond insoluble?

A

due to very strong covalent bonda between the atoms

50
Q

Structure of Graphite

A

3 covalent bonds per carbon atom
Layers of hexagons
Weak intermolecular forced between layes
crystalline structure
One free electron per carbon aton

51
Q

1.

Properties of graphite

A

High melting ang boiling points
Conducts electricity
Solid at room temp
Soft
Insoluble in water

52
Q

Metallic Bonding

A

Metals in solids have their outershells de-localised. The sharing of these de-localised electrons creatre strong metallic bonds

53
Q

What is the formula for Ammonia?

A

NH₃

54
Q

What is the formual for Ammonium Ion

A

NH₄⁺

55
Q

What is the formula for Nitrate ion?

A

NO₃⁻

56
Q

What is the formula for sulfate ions?

A

SO₄²⁻

57
Q

WHat is the formula for cabonate ions?

A

CO₃²⁻

58
Q

What does the ball on fire hazard mean?

A

Oxidising
Provides oxygen which allows other materials to burn more fiercely

E.g Liquid oxygen

59
Q

What does the exclamation mark hazard mean?

A

Harmful
Can cuase irritation, reddening or blistering of the skin

E.g Bleach

60
Q

What does the tree and dead fish hazard mean?

A

Environmental hazard
harmful to organisms and to the environment

E.g Mercury

61
Q

What does the Fire on a line Hazard mean?

A

Highly Flammible
Catches fire easily

E.g Petrol

62
Q

What does the skull hazard mean?

A

Toxic
Can cause death if consumed, absorbed, or inhailed.

E.g Hydrogen Cyanide

63
Q

What is the test tube and hand hazard?

A

Corrosive
Destroys materials, including living tissues (skin)

E.g Concentrated sulfuric acid

64
Q

What was John Dalton’s theory of atoms?

A

Solid spheres, Different spheres made up different elements

19th century

65
Q

What was J.J Thompsons theory of the atom?

A

The Plum Pudding
He mesured charge and mass and concluded that an atom must contain smaller, negatively charged particles (electrons)

1897

66
Q

What did the Plum pudding model look like?

A

Spherical positively charged pudding with smaller electrons in it

67
Q

What was the gold foil experement?

A

Ernest rutherford and his students, Hans Geiger and Ernest marden.
Fired positively charged alpha particles at a thin sheet of gold

1909

68
Q

How did the gold foil experement disprove the plum pudding model?

A

Based on the plum pudding model, the alpha particles would pass right through the sheet or be slightly deflected at most.
Some were delflected more than expected.

69
Q

How did the Nuclear atom model form from the gold foil experement?

A

Rutherford theorised that there was a tiny, positively charged nucleus at the centre. This would reason the alpha particles were deflected more than expected.

70
Q

How did Neils Bohr refign the theory of the atom?

A

Bohr suggested that electrons are in fixed shells or orbits, with fixed energy levels.

70
Q

How are ionic bonds held together?

A

They are strongly atttracted by electrostatic forces in the oppositely charges ions

71
Q

Ionic bonds vs Ionic compounds

A

Ionic compounds are the entire thing, molecules
Ionic bonds are the forces that hold them together

72
Q

What structure do ionic compounds have?

A

Regular lattice / Giant ionic lattice

73
Q

molecules

A

Groups of atoms

74
Q

What size are simple molecules?

A

10x-10 m

75
Q

How are simple molecules held together?

A

The atoms within are held together by very strong covalent bonds
But the molecules are held together by weak forces of attraction

76
Q

What state is a simple molecule at room temp?

A

Liquid or gas

77
Q

Properties of simple molecules

A

Very low melting and boiling points as only the intermolecular forces need to be broken
No conduction as no delocalised electron

78
Q

Polymers

A

long chains of covalently bonded atoms

79
Q

Graphene

A

1 layer of graphite
1 atom thick, making it 2d

80
Q

Fullerene shape

A

Molecules of carbon, shaped like closed tubes or hollow balls. Mainly made up of carbon atoms arranges in 6,5,7s shapes.

81
Q

Fullerene uses

A

Can be used to cage other molecules, this can be used to deliver drugs directly to the cells in a body
Huge surface area, so can be used as industrial catalysts

82
Q

Nanotubes

A

Fullerenes, cylinders of graphene
conduct electricity
high tensile strength
used on tennis rackets to strengthen them

83
Q

Simple molecular substances vs giant covalent

A

Simple molecular - Covalent compound held together by weak intermoleculer forces
Giant covalent - A massive compound of chained covalent bonds

84
Q

What structure are metals?

A

Giant

85
Q

What happens in metallic bonding?

A

The electrons in the outer shell of the metal are de-localised

86
Q

What bonds are in metallic bonding?

A

Strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons

These hold the metal atoms in a regular structure

87
Q

WHat kind of compounds are held together by metallic bonding?

A

Metallic elements and alloys

88
Q

What produces the characteristics in Metallic bonds?

A

The de-localised electrons

89
Q

How strong are Metallic bonds?

A

The electrostatic forces between the metal ions and the de-localised sea of electrons are very strong, so need alot of energy to be broken

90
Q

What are the physical properties of most metallic bonds?

A

high melting and boiling points
shiny solids at room temp
in soluble in water
dense in structure compared to non metals
malleable as layers can slide
good conductors

91
Q

Non-metals general characteristics

A

dull, brittle
lower boiling points
dont conduct
lower boiling points

Chemistry (7 decks)

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