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Chemistry Flashcards

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1
Q

What are the 3 states of Matter?

A

solid, liquid, gas

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2
Q

How does a solid change to a liquid?

A

melting

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3
Q

How does a solid change to a gas?

A

sublimation

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4
Q

How does a liquid change to a solid?

A

freezing

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5
Q

How does a liquid change to a gas?

A

boiling(evaporation)

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6
Q

How does a gas change to a liquid?

A

condensation

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7
Q

What is a melting point?

A

the temperature at which a substance changes from a solid to a liquid

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8
Q

What is a boiling point?

A

the temperature at which a substance changes from a liquid to vapour

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9
Q

Why do some substances melt easily whilst others need lots of energy?​

A

Because the amount of energy needed to change state depends on the strength of forces between the particles of the substance.

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10
Q

What is a chemical bond?

A

the forces of attraction that bind atoms together in a molecule.

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11
Q

How are chemical bonds formed?

A

when valence electrons, the electrons in the outermost electronic “shell” of an atom, interact. ​

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12
Q

What are the 3 types of chemical bonds?

A

ionic,covalent, metallic

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13
Q

What is an Ionic Bond and example?

A

Electrons are transferred from metal to non-metal atoms to form positive and negative ions. These oppositely-charged ions are attracted to each other.​(e.gNaCl)

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14
Q

What is a Covalent Bond and example?

A

A covalent bond is a shared pair of electrons that occurs in non-metal atoms. (e.g. I2, CH4)​

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15
Q

What is a Metallic Bond?

A

The metallic bond is the strong electrostatic force of attraction between the positive metal ions and the ‘sea’ of delocalised electrons.​(Cu)

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16
Q

Which chemical bond will form in brass?

A

Metallic Bond

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17
Q

Which chemical bond will form in Nitrogen Chloride?

A

Covalent Bond

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18
Q

Which chemical bond will form in Sulfur Dioxide?

A

Covalent Bond

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19
Q

Which chemical bond will form in Sodium Fluoride?

A

Ionic Bond

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20
Q

What is an Ion?

A

It is a charged atom caused by metals or non-metals transferring electrons.

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21
Q

What is a metal ions charge when losing an electron and what are they called?

A

Positively Charged they are called cations

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22
Q

How are the non-metal ions charged when gaining an electron and what are they called?

A

Negatively Charged they are called anions

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23
Q

How are the negative and positive bonds attracted to each other in Ionic Bonding?

A

Electrostatic Attraction

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24
Q

How do Covalent Bonds bond?

A

by sharing electrons

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25
Q

What is a Diatomic Molecule?

A

contain two atoms that are chemically bonded.

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26
Q

What are the 6 Diatomic Molecules?

A

Hydrogen,Nitrogen,Oxygen,Fluorine,Bromine,Iodine

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27
Q

What is a simple covalent molecule?

A

Molecules that consist of just a few atoms held together by covalent bonds

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28
Q

What is the approximate radius of an atom in satndard form?

A

1 × 10 (-10 m)

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29
Q

How do you work out an Ionic Compound?

A
  1. Write down the symbol for each element – the metal is always written first.​
  2. Calculate the charge for each type of ion.
  3. Write the rate of the ions.
  4. Use the ratio to write down the formula of the ionic compound.​

​

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30
Q

Why is Nitrogen a gas at room temperature?

A

Because it has weak intermolecular forces which makes it a gas.

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31
Q

What is a Polymer?

A

Polymers are very large molecules made from repeating units called monomers .

​

​

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32
Q

In general which metals would you expect to have the highest melting point Group 1 or 2? ​

A

Group 2 have higher melting points and boiling points – this is because they have 2 spare electrons and therefore there is a greater electrostatic force of attraction. ​

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33
Q

Give me 5 properties of metals?

A

High Density,Hard,Lustrous,High Tensile Strength,High Boiling and melting point,Ductile,Malleable,good conductors of heat and electricity

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34
Q

Who made the modern periodic table?

A

Dmitri Mendeleev

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35
Q

What are the 2 types of Ions?

A

Cations and Anions

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36
Q

What group is Halogens?

A

Group 7

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37
Q

What group is Noble Gases?

A

Group 0

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38
Q

Why are Noble Gases unreactive?

A

They are already stable as they already have full outer electron shells.​

39
Q

How many electrons do halogens on their valence electrons?

A

they have 7 electrons meaning they are reactive

40
Q

Are halogens metals or non-metals?

A

non-metals

41
Q

What colour is Fluorine at room temperature?

A

It is a yellow gas

42
Q

What colour is Chlorine at room temperature?

A

It is a Greenish-yellow gas

43
Q

What colour is Bromine at room temperature?

A

It is a red-brown liquid

44
Q

What colour is Iodine at room temperature?

A

It is a blue-black solid

45
Q

Why do Halogens exist as Diatomic Molecules?

A

Becuase each halogen is short of an electron on their outer shell so it shares its unpaired electron with another atom of the same halogen to form diatomic molecules

46
Q

Why do all halogens react the same way?

A

Because they all have 7 electrons in their outer shell​

47
Q

Why does the reactivity of halogens decrease going down the group?

A

Because the atomic number gets larger going down the group resulting in more electrons shielding the nucleus and the further the outer shell from the nucleus the harder it is to attract another electron to complete the shell.

48
Q

How do Halogens react with non-metals?

A

Unlike their reactions with metals, halogens share electrons with non-metals, and so react to form covalent compounds.​

49
Q

What is a displacement reaction?

A

A displacement reaction is one where a more reactive element takes the place of a less reactive element in a compound.​

50
Q

What group is alkali metals?

A

Group 1

51
Q

Why does the reactivity of alkali metals increase going down the group?

A

The atomic number increases resulting in the outer shell being further away from the nucleus which means more electrons are shielding the nucleus and the further the electrons is from the positive nucleus the easier it is lost in reactions.

52
Q

What do high densities and high melting points require?

A

Low Reactivity

53
Q

What does Pure mean?

A

a substance is pure if it is a single element or compound, not mixed with any other substance.​

54
Q

Are mixtures pure true or false?

A

False - mixtures are not pure

55
Q

What does a pure substance melt or boil at?

A

A pure substance will boil at a very precise melting and boiling point with a range of less than 2 degrees.

56
Q

What does a mixture melt or boil at?

A

It melts or boils over a much wide range often more than 5 degree range

57
Q

What is a formulation?

A

A formulation is a mixture that has been designed as a useful product. ​

58
Q

How are formulations made?

A

by mixing the components in carefully measured quantities to ensure that the product has the required properties.​

59
Q

What is a giant covalent structure?

A

a three-dimensional structure of atoms that are joined by covalent bonds.

60
Q

Giant covalent structure examples?

A

diamond, graphite (types of carbon) and silicon dioxide (silica)

61
Q

What is an ionic lattice?

A

When oppositely charged ions arrange themselves into a repeating pattern of alternating charges.

62
Q

What is a giant ionic lattice?

A

In a giant ionic lattice, there are strong electrostatic forces of attraction acting in all directions between the oppositely charged ions.

63
Q

What is a Mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together.

64
Q

What are the 2 types of mixtures

A

Heterogenous, Homogenous

65
Q

What is a Homogenous mixture?

A

a homogeneous mixture the particles of each substance are evenly spread throughout the mixture.​

E.g. Milk, squash, brass.​

66
Q

What is a Heterogenous mixture?

A

In a heterogeneous mixture the particles of each substance are not evenly spread throughout the mixture.​

E.g. Sand and water, a bag of sweets.​

67
Q

What is a Solvent?

A

A substance that can dissolve something.

68
Q

What is a Solute?

A

The thing that is dissolved by the solvent.

69
Q

What is a Solution?

A

A solute dissolved in a solvent makes a SOLUTION

70
Q

What is filtering used for?

A

to separate soluble solids from insoluble solids (e.g sand in water)

71
Q

What is Crystallisation used for?

A

to obtain a soluble solid from a solution (e.g salt crystals from salty water)

72
Q

What is Evaporation used for?

A

to obtain a solute from a solution

73
Q

What is Simple Distillation used for?

A

to obtain a solvent from a solution

74
Q

What is Fractional Distillation?

A

Used to separate mixtures in which the components have different boiling points.

75
Q

What 2 phases are there in chromatography?

A

Mobile Phase and Stationary Phase
In chromatography, a mobile phase (liquid) moves through a stationary phase (paper or TLC plate).​

76
Q

What is Chromatography?

A

Used to separate the different soluble, coloured components of a mixture.

77
Q

What is a mobile phase in chromatography?

A

The solvent that carries chemicals from a sample through a chromatographic column or sheet .

78
Q

What is a stationary phase in chromatography?

A

The medium through which the mobile phase passes in chromatography.​

79
Q

What is an aqueous in chromatography?

A

An aqueous solution is a solution in which water is the solvent.​

80
Q

What is a non-aqueous in chromatography?

A

A solution in which a liquid other than water is the solvent (alcohol)​

81
Q

What is retention time in chromatography?

A

this is the time taken for a component in a mixture to pass through the stationary phase.​

82
Q

What is a reference material in chromatography?

A

Known chemicals used in analysis for comparison with unknown chemicals. ​

83
Q

What is a solvent front in chromatography?

A

the furthest position reached by the solvent during chromatography.​

84
Q

What is a locating agent in chromatography?

A

A chemical used to show up colourless spots on a chromatogram​

​

85
Q

What type of ions do the following form:
1. Sodium
2. Hydroxide
3. Sulfate
4. Oxygen

A
  1. Na+
  2. Ho-
    3.SO2 -4
  3. o -2
86
Q

What do we call rows in the Periodic table?​

A

periods or series

87
Q

What do we call columns in the Periodic table?​

A

Groups

88
Q

What do we call the elements in the central block of the Periodic table?​

​

A

Transition Metals

89
Q

What did John Newlands discover?

A

In 1864 he found that every eight elements had similar properties and called this the law of octaves he put it in atomic mass (called newlands octaves)

90
Q

What did Dmitri Mendeleev discover?

A

the periodic table

91
Q

Why did Mendeleev leave gaps in his “table of elements”

A

they predicted the properties of so far undiscovered elements.

92
Q

how are the elements arranged in the modern periodic table?

A

According to their atomic number

93
Q

how are the elements arranged in the early periodic table?

A

According to their atomic mass

Combined Science (4 decks)

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