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Chemistry > (Topic 1) Atomic Structure And Periodic Table (CGP Book) > Flashcards

(Topic 1) Atomic Structure And Periodic Table (CGP Book) Flashcards

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1
Q

What is the radius of an atom?

A

0.1 nm

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2
Q

What do atoms contain?

A

Protons, neutrons, and electrons

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3
Q

Where is the nucleus located?

A

Middle of the atom

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4
Q

What does the nucleus contain?

A

Protons and neutrons

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5
Q

What is the radius of a nucleus?

A

1 x 10*14

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6
Q

What charge does the nucleus have?

A

A positive one

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7
Q

Where is the mass of an atom concentrated?

A

At the nucleus

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8
Q

What is the charge of a proton?

A

+1

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9
Q

What is the charge of a neutron?

A

0

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10
Q

What is the charge of an electron?

A

-1

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11
Q

What is the relative mass of a proton?

A

One

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12
Q

What is the relative mass of a neutron?

A

One

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13
Q

What is the relative mass of an electron?

A

Zero or very small

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14
Q

How do electrons move around?

A

They move around the nucleus in outer electron shells

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15
Q

What is the charge of an atom?

A

Neutral, this is because they have the same number of protons and electrons

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16
Q

What is an ion?

A

An atom or a group of atoms that has lost or gained electrons

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17
Q

What does the nuclear symbol of an atom tell you?

A

It’s atomic number and mass number

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18
Q

What does the atomic number show you?

A

How many protons there are?

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19
Q

What does the mass number show you?

A

The number of protons and neutrons in the atom

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20
Q

How do you find the number of neutrons in an atom?

A

Subtract the atomic number from the mass number

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21
Q

What is an element?

A

A substance made up of atoms that all have the same number protons in the nucleus

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22
Q

What is an isotope?

A

Elements that have the same number of protons but a different number of neutrons

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23
Q

What are compounds?

A

Substances formed from two or more elements, the atoms of each are in fixed proportions throughout the compound and are held together by chemical bonds

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24
Q

What happens in a compound which is formed from a metal and nonmetal?

A

The metal atoms lose electrons to form positive ions
The non-metal atoms gain electrons to form negative ions
The opposite charges of the ions means they are strongly attracted to each other. This is known as ionic bonding.

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25
Q

What happens in a compound that is formed from non-metals?

A

Molecules are formed
Each atom shares an electron with another atom
This is called covalent bonding

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26
Q

How can mixtures be separated?

A

Filtration, crystallisation, simple distillation and fractional distillation

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27
Q

What is crude oil?

A

A mixture of different length hydrocarbon molecules

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28
Q

Process of paper chromatography?

A

Draw line near bottom of a sheet of filter paper
Add spot of ink to line and place sheet in a beaker of solvent
Make sure ink is not touching solvent
Solvent seeps up paper carrying ink with it
Each different diet in ink will move paper at a different rate so will separate forming a separate spot
If any dyes are insoluble, they will stay on the baseline
When solvent has reached top of paper, take it out and leave to dry resulting in a chromatogram

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29
Q

When can filtration be used?

A

If your product is an insoluble solid that needs to be separated from a liquid reaction mixture

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30
Q

What does filtration do?

A

Separate insoluble solids from liquids

31
Q

What does soluble mean?

A

A solid that can be dissolved

32
Q

What are two methods for separating a soluble salt from a solution?

A

Evaporation and crystallisation

33
Q

Process of evaporation?

A

Pour solution into evaporating dish
Slowly heat solution, solvent will evaporate and solution will get more concentrated. Eventually crystals will start to form
Keep heating evaporating dish until dry crystals are left

34
Q

Process of crystallisation?

A

Call solution into evaporating dish and gently heat solution, some of solvent will evaporate and solution will get more concentrated
Once some of solvent has evaporated remove dish from heat and leave solution to cool
Salt should start to form crystals as it becomes insoluble in cold highly concentrated solution
Filter crystals out of solution and leave them in a warm place to dry

35
Q

What is simple distillation used for?

A

To separate out solutions

36
Q

Process of simple distillation?

A

Solution is heated, part of solution that has lowest boiling point evaporates first
Vapour is then cooled, condenses and is collected
Rest of solution is left in flask

37
Q

What is fractional distillation used for?

A

To separate a mixture of liquids

38
Q

Process of fractional distillation?

A

Put mixture in flask and stick a fractionating column on top then heat it
Different liquids have different boiling points so will evaporate at different temperatures
Liquid with lowest boiling point evaporates first
Liquids with higher boiling points further up the fraction it in column before running down to the flask

39
Q

When and what did John Dalton say about the atomic structure?

A

Start of 19th century described atoms as solid spheres and said that different spheres made up different elements

40
Q

When and what did JJ Thompson say about the atomic structure?

A

1897, he concluded from his experiments that atoms were not solid spheres
Measurements of charge and mass showed that an atom must contain even smaller negatively charge particles
He called his theory the plum pudding model

41
Q

What did the plum pudding model show?

A

The atom is a ball of positive charge with electrons stuck in it

42
Q

When and what did Ernest Rutherford say about the atomic structure?

A

In 1909, conducted Alpha particle scattering experiments
Fired positively charged alpha particles at an extremely thin sheet of gold
Most of particles went straight through some of deflected, and a small number with deflected backwards, this disproved the plum pudding model

43
Q

What was Rutherford’s new model of the atomic structure called?

A

The nuclear model
Demonstrate a tiny positively charged nucleus at centre, where most of mass is concentrated
A cloud of negative electrons surround the nucleus most of atom is empty space

44
Q

What did Niels Bohr say about the atomic structure?

A

Suggested all electrons were contained in shells which orbit the nucleus

45
Q

What did James Chadwick state about the atomic structure?

A

Discovered neutral particles in nucleus known as neutrons

46
Q

How were elements arranged in the early 1800s and why?

A

By atomic weight
Scientists had no idea of atomic structure or of protons, neutrons of electrons

47
Q

What was wrong with early periodic tables?

A

They were incomplete and some elements placed in wrong group

48
Q

When and what did Dimitri Mendeleev state about the periodic table?

A

Took 50 non-elements and arrange them into his table of elements and left various gaps
Elements mainly in order of atomic weight but also by their properties
When elements were found, they fitted the gaps he left

49
Q

How is the modern periodic table organised?

A

Elements laid out in order of increasing atomic number, this means there are repeating patterns in properties of elements
Vertical column are called groups and Represent elements with similar properties
Group tells you how many electrons in outer shell
Rows are called periods

50
Q

What are metals?

A

Elements which can form positive ions when they react

51
Q

How do elements gain a full outer shell?

A

They react and either lose, gain or share electrons

52
Q

How do metals bond?

A

Metallic bonding

53
Q

Properties of metals?

A

They are strong but malleable
Great at conducting heat and electricity
Have high boiling and melting points

54
Q

Properties of nonmetals?

A

Tend to be dull looking
More brittle
Aren’t always solids at room temperature
Don’t generally conduct electricity
Often have a lower density

55
Q

Properties of transition metals?

A

Good conductors of heat and electricity
Very dense, strong and shiny
Can have more than one ion
Often coloured
Often make good catalysts

56
Q

Where are the transition metals found?

A

Groups two and three

57
Q

What are group one elements known as?

A

The alkali metals

58
Q

Properties of alkali metals?

A

Reactive
Soft
One electron in outer shell
Low density

59
Q

What happens as you go down group one?

A

Increasing reactivity
Lower melting and boiling points
Higher relative atomic mass

60
Q

What happens when alkali metals react with water?

A

React vigourously to produce hydrogen and metal hydroxides

61
Q

What is a metal hydroxide?

A

Compounds that dissolve in water to produce alkaline solutions

62
Q

How do group one elements react with chlorine?

A

React vigourously when heated in chlorine gas to form white metal chloride salts

63
Q

How do group one elements react with oxygen?

A

React with oxygen to form a metal oxide

64
Q

What are group 7 elements known as?

A

The halogens

65
Q

What colour gas is fluorine?

A

Yellow

66
Q

What colour gas is chlorine?

A

Green

67
Q

What colour gas is bromine?

A

Red/brown

68
Q

What colour is iodine?

A

A dark grey crystalline solid
Purple vapour

69
Q

What happens as you go down group 7?

A

Less reactive as it is harder to gain an extra electron because the outer shell is further from the nucleus
Higher melting and boiling points
Higher relative atomic masses

70
Q

How do halogen atoms share electrons with other non metals?

A

Covalent bonding

71
Q

How do halogens bond with metal?

A

Ionic bonding

72
Q

What are group 0 elements known as?

A

Noble gases

73
Q

Properties of noble gases?

A

Stable as have full outer shell
Colourless gases
Non-flammable

74
Q

What happens as you go down the noble gases?

A

Boiling points increase because of an increase in number of electrons in each atom leading to greater intermolecular forces
Relative atomic mass increases

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