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Chemistry > TOPIC C1 > Flashcards

TOPIC C1 Flashcards

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1
Q

Describe the structure of the neuclues

A

It’s in the middle of the atom
Contains protons and neutrons
It’s positively charged because of the protons

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2
Q

Describe the electrons

A

It’s negatively charged and tiny but they cover a lot of space
Volume of their orbits the determines the sizes of the atom

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3
Q

What does the nuclear symbol tell you

A

It tells you it’s atomic and mass number

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4
Q

What does the atomic number tell you

A

Tell us you how may protons there are

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5
Q

What does the mass number tell you

A

It tells you the total number of the protons and neutrons in the atoms

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6
Q

How do U get the totally number of neutrons

A

You just subtract the atomic number from the mass number

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7
Q

What is a substance called when it has the same number of protons

A

An element. There are about 100 different elements

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8
Q

What are Isotopes

A

They are different forms of the same element they have the same number of protons but different numbers of neutrons

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9
Q

How are compounds formed

A

When elements react and atoms combine with other atoms

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10
Q

How are compounds formed

A

They are formed from two or more elements

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11
Q

How do we separate elements

A

A chemical reaction needs to take place

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12
Q

What type of bonding does she he compound forms

A

Covalent bonding- each atoms shares an electron with another atom

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13
Q

What are the properties of a compound

A

The properties are totally different from its original elements

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14
Q

What does a formula show

A

A formula shows what atoms are in a compound

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15
Q

What two parts can a mixture be

A

Either elements and compounds

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16
Q

How can mixtures of elements or compounds be separated

A

Such as filtration, crystallisation , smile distillation, fractional distillation and chromatography

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17
Q

What are the properties of a mixture

A

It’s the the properties of the separate parts

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18
Q

What were the elements arranged by in 1800s

A

By the Atomic Mass

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19
Q

What were the only two ways that elements were separated into

A

1) their physical and chemical properties

2) their relative atomic mass

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20
Q

What are the elements arranged in

A

Atomic number

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21
Q

Back then, what was the only thing the could measure

A

Relative atomic mass

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22
Q

Who left gaps in the early period table

A

Dmitri Mendeleev

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23
Q

Why did Dmitri Mendeleev leave gaps in the periodic table

A

To make sure that elements wot similar properties stayed in the same groups

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24
Q

What did same of the gaps indicate

A

They indicated the existence of undiscovered elements and allowed Mendeleev to predict what their properties might be

25
Q

How are the elements laid out in the early periodic table

A

By the increasing atomic number

26
Q

What is the periodic table helpful for

A

They hate helpful for working out the metals(found to the left)and which are non-metals(found to the right)

27
Q

How are elements set out to form a column

A

Similar properties

28
Q

What does the group number tell you

A

They tell you how much electrons there are in the outer shell

29
Q

Why are elements put into similar properties

A

Because they are likely to react in the same way

30
Q

What can u predict from the properties of one element

A

You can predict the properties of other elements in the group

31
Q

What does the way the atoms react depend on

A

The number of the electrons in their outer shell

32
Q

What are the rows called

A

They are called periods

33
Q

What type of element can be formed by metals

A

They form a positive ions when they reach

34
Q

Are most of the elements in the periodic table metals or non-metals

A

Metals

35
Q

How do atoms react with each other to make a full outer shell

A

By losing,gaining,or sharing electrons

36
Q

What type of bonding do all the metals have

A

All the metallic bonding shock causes them to have a similar basic physical properties

37
Q

What are the physical properties of metal

A

They are strong( hard to break)but can be bent or hammered into a different shapes
Metals conduct heat and electricity
They have highly boiling points

38
Q

The properties of a non-metals

A

They don’t have metallic bonding
They are full looking
More brittle, they aren’t always solid at a room temperature
They don’t conduct electricity and often have a lower density

39
Q

What are the alkali metals

A

Lithium,sodium,potassium,rubidium,caesium and francium

40
Q

What are the group 1 elements like

A

They were reactive,soft metals

41
Q

What makes group one elements reactive

A

They all have one electron in their outer shell which makes them very reactive

42
Q

What is trend like in group one

A

Lower boiling and melting point

Higher relative mass

43
Q

What are group 7 elements shown as

A

Halogens

44
Q

What are the trends of the group 7

A

As you go down they:

1) they become less reactive
2) high melting and boiling point
3) highly relative atomic masses

45
Q

Why do all of the elements of group 7 react in similar ways

A

This is because they all have seven electrons electrons in their outer shell

46
Q

What are the group 0 elements known as

A

Noble gases

47
Q

Explain the benefits of the group 0 having a full outer-shell

A

This means the shells are stable and they don’t need to give up or gain electrons to become more stable

48
Q

What are group 0 like at a room temperature

A

They are colourless gases at a room temperature

49
Q

Are noble gases flammable

A

No they are inert

50
Q

Describe what the properties are like in the noble gases

A

The boiling point of the noble gases increases as you move down the group along with increasing relative atomic mass

51
Q

What type of bonding does group one react to form

A

Ionic compounds

52
Q

Fluorine

A

Very reactive

Poisonous yellow gas

53
Q

chlorine

A

Fairly reactive

Poisonous dense green gas

54
Q

Bromine

A

Very dense

Poisonous red-brown volatile liquid

55
Q

Iodine

A

Very dark grey crystalline solid

Or a purple vapour

56
Q

What colour are all the noble gases at room temperature

A

All group elements in group 0 are colourless gases

57
Q

Are nobles gases flammable

A

They are non-flammable as they are inert

58
Q

What does it mean is they nobles gases are bonded together

A

They exist as monatomic gases-single atoms not bonded with each other

59
Q

What causes the increase of the boiling point

A

It’s due to an increase in the number of electrons in each atoms leading to greater intermolecular forces

Chemistry (5 decks)

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