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Chemistry Flashcards

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1
Q

Density

A

How easily it sinks

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2
Q

Boiling point

A

The temperature the substance changes from a liquid to a gas

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3
Q

Melting point

A

The temperature where it changes from a solid to liquid

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4
Q

Features of a pure substance

A

Fixed melting point

Fixed boiling point

Contains only one type of atom

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5
Q

Energy of a substance and temperature of a substance at its melting point (what happens to it)

A

Energy goes into changing the phase of a substance

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6
Q

Element

A

A substance made up of only 1 type of atom

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7
Q

Atom

A

Smallest part of an element to exist

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8
Q

Molecule

A

A small group of atoms that are covalently bonded

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9
Q

Compound

A

A pure substance made of 2 or more different elements chemically bonded

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10
Q

Mixture

A

A mixture contains 2 or more substance not chemically joined together

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11
Q

What symbol do these elements have

Gold

Lead

Silver

A

Gold - Au

Lead - Pb

Silver - Ag

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12
Q

Iron sulphide word equation

A

Fe + S = FeS

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13
Q

Classify elements

A

Elements can be classifed as metals, non-metals and metalloids

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14
Q

Classify compounds (what type are they)

A

Compounds are classifed as inorganic and organic compounds

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15
Q

What happens to mass in a chemical reaction

A

Mass is conserved

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16
Q

Relative mass of subatomic particles

A

Protons 1

Neutrons 1

Electrons -1

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17
Q

Why is mass conserved in a chemical reaction

A

No new atoms have entered or left the system so the mass is conserved

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18
Q

Significance of chemical symbols used in formulae and equations

A

Useful to write a chemical formula of any compound in a short form

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19
Q

How mass may appear to change in a chemical reaction

A

If a gas escapes the total mass will look as if it has decreased

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20
Q

Phosphorus

A

P

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21
Q

John Dalton’s model of atom

A

Billiard ball model

Atoms were of a ball like structure

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22
Q

John Jacob Berzelius model of atom

A

Intoduced simple alphabet characters to symbolize each element

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23
Q

Joseph John Thomson model of atom

Plum pudding model

A

A sphere with protons and electrons mixed together

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24
Q

Ernest Rutherford model of atom

Nuclear model

A

An outer shell with protons and the nucleus at the centre and electrons surrounding the nucleus

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25
Q

Niels Bohr atom model

A

Planetary model

Electrons spin around nucleus in orbits

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26
Q

Difference between plum pudding model and nuclear model

A

Nuclear model has a positively charged nucleus

Plum pudding - electrons and protons mixed together

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27
Q

How evidence from scattering experiments changed the model of atom

A

Results from alpha scattering led the plum pudding model replaced by the nuclear model

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28
Q

Describe atoms using the atomic model

A

Atoms contain electrons protons and neutrons

Electrons orbit the nucleus in energy levels

Protons and neutrons found in nucleus

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29
Q

Why model of atom changed overtime

A

Scientists changed the model so it could explain new evidence

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30
Q

How to describe familiar chemical equations

A

Reactants —–> products

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31
Q

Ion

A

Atom or a group of atoms with positive or negative charge as a result of having lost or gained one or more electrons

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32
Q

Why ions have a charge

A

The number of electrons doesn’t equal the number of protons in the atom

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33
Q

Isotopes

A

Forms of an element with the same number of protons but different number of neutrons

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34
Q

How to describe isotopes using atomic model

A

Atoms with different numbers of protons and nuetrons

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35
Q

What are the patterns in periodic table

A

Atomic radius

Mass number

Reactivity

36
Q

Why can we be sure that there are no missing elements in first 10 elements of periodic table

A

Any atom with 6 protons is carbon, it cannot be anything else

All the other elements have a number of protons which no other element has the same number

37
Q

How to work out atomic number of an element

A

Number of protons = atomic number

Number of electrons = atomic number

38
Q

How to work out number of neutrons

A

Mass number - atomic number

39
Q

How to work out mass number

A

Number of neutrons + number of protons

40
Q

Size of an atom in standard form

A

-10
1 x 10 m

41
Q

Why chlorine does not have a whole mass number

A

Due to involvment of isotopes

42
Q

Why elements in same group react in a similar way

A

They have similar number of valence electrons

43
Q

What happens to electrons the further down the energy levels they go

A

Their energy increases the longer the line

44
Q

State relative mass of a nucleus

A

-15
10 m

45
Q

State maximum number of electrons in the first 3 energy levels

A

1st shell - 2

2nd shell - 8

3rd shell - 18

46
Q

How we can make predictions for how an element will react when given information on another element in the group

A

Elements in same group have similar chemical properties

There’s usually a pattern in their physical properties

47
Q

List the significant models for ordering the elements

A

Periodic table

Relative atomic masses

48
Q

How the elements are ordered in the perioic table in groups and periods

A

In order of increasing atomic number

49
Q

Why ordering of elements has changed over time

A

Henry Moseley rearranged the elements to their atomic numbers

This helped explain disparities in earlier versions that used atomic mass

50
Q

Why the periodic table was a breakthrough in how to order the elements

A

Mendeleev found out not all elements have been discovered yet

He left gaps on the table to place elements scientists didn’t know yet

51
Q

Define groups and periods in the perioidc table

A

Groups - columns in the periodic table

Periods - rows

52
Q

How electronic structure is linked to periodic table

A

Number of electrons in the outermost shell of an element is represented in the periodic table as group number that element is in

53
Q

Why noble gases are unreactive

A

The atoms of noble gases have complete outer shells so they don’t lose, gain or share electrons making them unreactive

54
Q

Boiling point and melting point trend in melting points

A

Boiling point - increases

Melting point - decreases

55
Q

How electronic structure of metals and non-metals are different

A

Atoms of metal elements give away electrons in their reactions to form positive ions

Electrons in non-metals are localized in covalent bonds

56
Q

How electronic structure of metals and non-metals affects their reactivity

A

Atoms of elements give away electrons in their reactions

Atoms of non-metals gain electrons in some of their reactions

57
Q

In terms of electronic structure how elements in periodic table are arranged

A

By increasing atomic number

58
Q

How to use periodic table to make predictions about the electronuc structure and reaction of elements

A

The electronic structure of an atom can be predicted from its atomic number

59
Q

First 3 elements in group 1

A

Hydrogen

Lithium

Sodium

60
Q

Features of group 1 metals

A

Soft

Silver metals

Low density

Low melting point

Highly reactive

61
Q

What happens when group 1 metals react with non-metals

A

Group 1 metals form ions with +1 charge

62
Q

Why the elements in group 1 react similarly

A

The elements in group 1 all have 1 electron in their outer electron shell

This means they share similar properties and behave similarly in chemical reactions

63
Q

Why first 3 elements group 1 float on water

A

Lithium sodium potassium are less dense than water

64
Q

How hydrogen and metal hydroxides are made when group 1 metals react

A

Hydrogen gas is given off and the metal hydroxide is produced

65
Q

Name the first 4 elements group 7

A

Fluorine

Chlorine

Bromine

Iodine

66
Q

How to recognise a halogen displacement reaction

A

The reaction mixture turns darker and iodine solution forms

67
Q

Why elements group 7 react similarly

A

They have the same number of electrons in their outer shell

68
Q

How group 1 metals are stored and safety precautions used when dealing with them

A

Should be stored in mineral oil or kerosene

Do not expose to air or water
Avoid contact with skin and eyes

69
Q

How Group 7 non-metals form ions with a −1 charge when they react with metals

A

When group 7 element takes part in a reaction its atoms each gain 1 electron forming a negatively charged ion

70
Q

Main properties of halogens

A

7 valence electrons

Halogens have 1 electron missing as they form negative ions

Highly reactive

71
Q

How to compare the reactivity of the Group elements

A

As you go down group 7 reactivity of halogen decreases

Electronic structure - the atomic mass of the halogen increases

72
Q

The trend in reactivity group 1

A

The reactivity increases as you go down the group

Electronic structure - the atoms get larger

73
Q

Use electronic structure to explain trends in physical and chemical properties of group 1

A

When an element in group 1 takes part in a reaction its atoms loses their outer electron and form positively charged ions

74
Q

Use electronic structure to explain trends in physical and chemical properties of group 7

A

The group 7 elements gain one more electron so they have a stable electronic structure

75
Q

Use the nuclear model to explain how the outer electrons experience different levels of attraction

A

Attraction between the nucleus and the outer electrons increases across a group because the proton number increases

76
Q

Why mercury is not a typical transition element

A

Neither the atom or its cations possess an incomplete d-subshell

77
Q

Chemical properties of transition metals and their compounds

A

Good conductors of heat and electricity

High melting points

Usually hard and tough

High density

78
Q

Justify the use of a transition metal

A

Used in construction materials

tools, vehicles

79
Q

Compare group 1 metals and transition

A

Transition metals are much stronger, denser and harder than group 1

80
Q

Why group 1 metals have different properties to transition metals

A

As 3d electrons delocalise the number of electrons involved in metallic bonding increases

81
Q

Trend in group 2 reactivity

A

Increases

Outer electons easier to remove

82
Q

Trend in group 6 reactivity

A

Decrease

Electronegativity decreases

83
Q

State the particles involved in ionic and covalent bonding

A

Covalent - a pair of electrons shared between 2 atoms

Ionic - a cation and an anion

84
Q

How a group 1 metal atom becomes a positive ion

A

When metals in group 1 lose 1 electron they become ions with a +1 charge

85
Q

Examples of how group 1 metal becomes positive ion

A

Lithium has 1 electron in its outer shell which it needs to lose and when losing this electron lithium becomes an ion

86
Q

Describe with an example how a group 7 non-metal becomes a negative ion

A

Fluorine will gain one electron to become a negative fluroide ion

-
F

87
Q

How a group 7 non-metal becomes a negative ion

A

Non-metals of Group 7 need to gain 1 electrons

Science (5 decks)

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