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Chemistry > TOPIC C1 > Flashcards

TOPIC C1 Flashcards

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
How are the elements laid out in the early periodic table
By the increasing atomic number
26
What is the periodic table helpful for
They hate helpful for working out the metals(found to the left)and which are non-metals(found to the right)
27
How are elements set out to form a column
Similar properties
28
What does the group number tell you
They tell you how much electrons there are in the outer shell
29
Why are elements put into similar properties
Because they are likely to react in the same way
30
What can u predict from the properties of one element
You can predict the properties of other elements in the group
31
What does the way the atoms react depend on
The number of the electrons in their outer shell
32
What are the rows called
They are called periods
33
What type of element can be formed by metals
They form a positive ions when they reach
34
Are most of the elements in the periodic table metals or non-metals
Metals
35
How do atoms react with each other to make a full outer shell
By losing,gaining,or sharing electrons
36
What type of bonding do all the metals have
All the metallic bonding shock causes them to have a similar basic physical properties
37
What are the physical properties of metal
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
The properties of a non-metals
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
What are the alkali metals
Lithium,sodium,potassium,rubidium,caesium and francium
40
What are the group 1 elements like
They were reactive,soft metals
41
What makes group one elements reactive
They all have one electron in their outer shell which makes them very reactive
42
What is trend like in group one
Lower boiling and melting point | Higher relative mass
43
What are group 7 elements shown as
Halogens
44
What are the trends of the group 7
As you go down they: 1) they become less reactive 2) high melting and boiling point 3) highly relative atomic masses
45
Why do all of the elements of group 7 react in similar ways
This is because they all have seven electrons electrons in their outer shell
46
What are the group 0 elements known as
Noble gases
47
Explain the benefits of the group 0 having a full outer-shell
This means the shells are stable and they don’t need to give up or gain electrons to become more stable
48
What are group 0 like at a room temperature
They are colourless gases at a room temperature
49
Are noble gases flammable
No they are inert
50
Describe what the properties are like in the noble gases
The boiling point of the noble gases increases as you move down the group along with increasing relative atomic mass
51
What type of bonding does group one react to form
Ionic compounds
52
Fluorine
Very reactive | Poisonous yellow gas
53
chlorine
Fairly reactive | Poisonous dense green gas
54
Bromine
Very dense | Poisonous red-brown volatile liquid
55
Iodine
Very dark grey crystalline solid | Or a purple vapour
56
What colour are all the noble gases at room temperature
All group elements in group 0 are colourless gases
57
Are nobles gases flammable
They are non-flammable as they are inert
58
What does it mean is they nobles gases are bonded together
They exist as monatomic gases-single atoms not bonded with each other
59
What causes the increase of the boiling point
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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