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What are all substances made from?

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Calculus

253 Terms

1

What are all substances made from?

atoms

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2

What is the smallest part of an element that can exist?

an atom

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3

Approximately how many different elements are there?

100

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4

Where are all of the elements shown?

The Periodic Table

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5

What are formed from elements by chemical reactions?

compounds

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6

What do chemical reactions always involve?

The formation of new substances

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7

What is this the definition of: Substances containing two or more elements chemically combined in fixed proportions

compound

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8

What is this the definition for: Something consisting of two or more elements or compounds not chemically combined together.

mixture

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9

Which processes can be used to separate mixtures?

Filtration, Crystallisation, Distillation, Chromatography, Fractional Distillation

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10

Before the discovery of electrons what were atoms thought to be?

Tiny spheres that could not be divided

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11

Which model was created due to the discovery of the electron?

The Plum-Pudding model

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12

What does the plum pudding model suggest about the atom?

That it is a ball of positive charge with negative electrons embedded in it

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13

What did the results from the alpha particle scattering experiment show?

That the mass of an atom was concentrated at the centre (nucleus) and the nucleus was charged

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14

How did Niels Bohr adapt the nuclear model

He suggested that electrons orbit the nucleus at specific distances

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15

What is the name given to small positively charged particles in the nucleus?

protons

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16

What did the experimental work of James Chadwick provided the evidence for?

neutrons

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17

What is the relative charge of the proton?

+1

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18

What is the relative charge of a neutron

0

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19

What is the relative charge of an electron

-1

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20

In an atom the number of electrons is equal to the number of

protons

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21

What is the atomic number of an element?

the number of protons

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22

All atoms of a particular element have the same number of?

protons

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23

Atoms of different elements have different numbers of

protons

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24

What is the radius of an atom?

0.1nm (1x10-^10m)

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25

How many times smaller is the radius of the nucleus compared to the atom

10,000

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26

What is the relative mass of a proton?

1

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27

What is the relative mass of a neutron?

1

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28

What is the relative mass of an electron?

Very small (1/2000)

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29

What is the mass number of an atom?

the sum of protons and neutrons

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30

What do we call atoms of the same element with different numbers of neutrons

isotopes

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31

Isotopes of an element have a different number of?

neutrons

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32

What is the relative atomic mass of an element?

The average values of the abundance of the isotopes of the element

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33

What is the maximum number of electrons that can be found on the lowest energy level?

2

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34

What is the maximum number of electrons that can be found on the second energy level?

8

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35

How are the elements in the periodic table arranged?

In order of atomic number

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36

What do we call a column in the periodic table?

groups

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37

What do we call rows in the periodic table?

periods

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38

What do elements in the same group in the periodic table have in common?

The same number of electrons in their outer shell

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39

Before the discovery of protons, neutrons and electrons how did scientists classify the elements?

Arranging them in order of their atomic weights

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40

How did Mendeleev overcome problems with creating a periodic table?

By leaving gaps for undiscovered elements

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41

Elements that react to form positive ions are

metals

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42

Elements that do not form positive ions are

non-metals

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43

The majority of elements are

metals

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44

Where are metals found on the periodic table?

To the left and bottom

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45

Where are non-metals found on the periodic table?

To the right and top

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46

What do we call the elements in Group 0?

The noble gases

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47

Why are Group 0 elements unreactive and do not easily form molecules?

They have stable arrangements of electrons

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48

How many electrons do the noble gases have in their outer shell (excluding Helium)

8

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49

What happens to the boiling point of the noble gases as you go down the group?

It increases

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50

Which noble gas has 2 electrons in the outer shell?

Helium

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51

What are the elements in Group 1 know as?

The alkali metals

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52

How many electrons are there in the outer shell of the alkali metals?

1

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53

How does the reactivity of the elements in Group 1 change as you go down the group?

It increases

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54

What is the general equation for the reaction of an alkali metal with chlorine?

Alkali metal + Chlorine → Metal chloride

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55

What is the general equation for the reaction of an alkali metal with water?

Alkali metal + Water → Metal hydroxide + Hydrogen

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56

What is the general equation for the reaction of an alkali metal with oxygen?

Alkali metal + Oxygen → Metal oxide

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57

What are the elements in group 7 known as?

the Halogens

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58

How many electrons do the Group 7 elements have in their outer shell?

7

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59

How are the halogens found?

In pairs of atoms

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60

As you go down Group 7 what happens to the boiling points of the elements?

It increases

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61

As you go down Group 7 what happens to the relative molecular mass of the elements?

It increases

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62

As you go down Group 7 what happens to the reactivity of the elements?

It decreases

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63

What will a more reactive halogen do to a less reactive halogen when in an aqueous solution of its salt?

Displace it

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64

What transition element is used in the Harber process?

Iron

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65

What transition element increases the decomposition of hydrogen peroxide to oxygen and water?

Manganese (IV) oxide

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66

What can the transition elements form?

Coloured compounds Ions with different charges

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67

What colour does Iron(II) hydroxide, Fe(OH)2

Pale green

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68

What colour does Iron(III) hydroxide, Fe(OH)3

Orange- brown

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69

What colour does Iron(III) oxide, Fe2O3

Red-brown

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70

What can the transition elements be used as?

Catalysts

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71

What are the transition elements?

Metals

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72

What are the main transition elements?

Chromium, Manganese, Cobalt, Nickle, Copper

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73

How should the transition elements be simplified as?

Cr, Mn, Fe, Co, Ni, Cu

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74

What do the transition elements have in common?

They have similar properties

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75

How do the transition elements differ from Group 1 metals?

-higher melting points

  • higher densities -Stronger and harder -Reactivity with oxygen, water and halogen Conducts electricity

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76

What type of bonding occurs between oppositely charged ions?

ionic bonding

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77

What type of bonding occurs between atoms which share pairs of electrons?

covalent bonding

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78

Which type of bonding is found in atoms which share delocalised electrons?

Metallic bonding

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79

Which type of bonding occurs in compounds formed from metals combined with non-metals?

Ionic bonding

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80

Which type of bonding occurs in most non- metallic elements?

Covalent bonding

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81

Which type of bonding occurs in compounds of non-metals?

Covalent bonding

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82

Which type of bonding occurs in alloys?

Metallic bonding

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83

What is transferred in ionic bonding?

electrons

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84

When a metal atom becomes positively charged what has it lost?

electrons

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85

What would be the charge of an ion formed from a Group 1 element?

+1

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86

What would be the charge of an ion formed from a Group 2 element?

+2

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87

What would be the charge of an ion formed from a Group 6 element?

-2

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88

What would be the charge of an ion formed from a Group 7 element?

-1

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89

What is an ionic compound?

a giant structure of ions

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90

What holds ionic compounds together?

Strong electrostatic forces of attraction between oppositely charged ions

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91

Name 2 covalently bonded substances with giant covalent structures

Diamond, Silicon dioxide

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92

Some covalently bonded substances have very large molecules, such as

polymers

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93

How are the atoms arranged in metals?

In a regular pattern

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94

What are the electrons in the outer shell of metal atoms like?

Delocalised

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95

What does delocalised electrons mean?

Electrons that are free to move around

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96

What are the three states of matter?

solid, liquid, gas

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97

What takes place at the melting point?

melting and freezing

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98

What takes place at the boiling point?

Boiling and condensing

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99

How does the strength of the forces between particles affect the boiling point?

The stronger the forces between the particles the higher the boiling point

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100

What are the limitations of the particle model?

  • There are no forces

  • All particles are represented as spheres

  • The spheres are solid

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