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Flashcards in TOPIC C1 Deck (59):
1

Describe the structure of the neuclues

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

2

Describe the electrons

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

3

What does the nuclear symbol tell you

It tells you it’s atomic and mass number

4

What does the atomic number tell you

Tell us you how may protons there are

5

What does the mass number tell you

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

6

How do U get the totally number of neutrons

You just subtract the atomic number from the mass number

7

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

An element. There are about 100 different elements

8

What are Isotopes

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

9

How are compounds formed

When elements react and atoms combine with other atoms

10

How are compounds formed

They are formed from two or more elements

11

How do we separate elements

A chemical reaction needs to take place

12

What type of bonding does she he compound forms

Covalent bonding- each atoms shares an electron with another atom

13

What are the properties of a compound

The properties are totally different from its original elements

14

What does a formula show

A formula shows what atoms are in a compound

15

What two parts can a mixture be

Either elements and compounds

16

How can mixtures of elements or compounds be separated

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

17

What are the properties of a mixture

It’s the the properties of the separate parts

18

What were the elements arranged by in 1800s

By the Atomic Mass

19

What were the only two ways that elements were separated into

1)their physical and chemical properties
2)their relative atomic mass

20

What are the elements arranged in

Atomic number

21

Back then, what was the only thing the could measure

Relative atomic mass

22

Who left gaps in the early period table

Dmitri Mendeleev

23

Why did Dmitri Mendeleev leave gaps in the periodic table

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

24

What did same of the gaps indicate

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