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NAT5 CHEMISTRY > Unit 1 > Flashcards

Unit 1 Flashcards

1
Q

What is the atomic number?

A

The number of protons in an atom’s structure.

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2
Q

What is the mass number?

A

The number of protons + neutrons in the atom’s nucleus.

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3
Q

Define Element.

A

Contains only one type of atom.

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4
Q

Define isotope.

A

Atoms with the same atomic number but different mass number.

(same number of protons as electrons, but different number of neutrons)

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5
Q

What is a molecule?

A

2 or more atoms chemically bonded together. (same or different)

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6
Q

Define a compound.

A

Two or more atoms of DIFFERENT elements chemically bonded together.

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7
Q

What is a mixture?

A

Two or more types of atoms, molecules, or compounds which AREN’T chemically bonded.

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8
Q

Define an ion.

A

A positively or negatively charged atom.

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9
Q

Define diatomic.

A

(to an element) An element/molecule which only occurs naturally in pairs.

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10
Q

What is a covalent bond and how is it held together?

A

A bond in which non-metal atoms are held together by a shared pair of electrons that are attracted to the positive nuclei of the atoms.

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11
Q

What is an ionic bond and how is it held together?

A

A bond between a metal and a non-metal, held together by oppositely charged ions.

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12
Q

What is group 1 called?

A

Alkali Metals

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13
Q

What is group 7 called?

A

The Halogens

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14
Q

What is group 0 called?

A

Noble Gases

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15
Q

What are the diatomic elements?

A

Iodine
Bromine
Chlorine
Fluorine
Nitrogen
Hydrogen
Oxygen

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16
Q

How are ionic bonds formed?

A

When a metal donates its outer electrons to a non metal

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17
Q

Do ionic substances conduct electricity and why?

A

Only when AQUEOUS (dissolved in water) or MOLTEN (melted)

This is because the ions are free to move.

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18
Q

Why do covalent molecules have low boiling and melting points?

A

Because their INTERMOLECULAR FORCES are weak and break easily.

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19
Q

How and why are ions formed?

A

Ions are formed when atoms lose or gain electrons in order to become stable.

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20
Q

Define a diatomic element.

A

An element which only naturally exists as a pair.

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21
Q

Why can graphite conduct but diamond can’t?

A

Graphite has delocalised electrons which move between layers, allowing electricity to flow.

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22
Q

What charge is the nucleus of an atom?

A

Positive

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23
Q

What are the four shapes of molecular bonds?

A

Linear
Angular
Trigonal Pyramidal
Tetrahedral

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24
Q

What is formula mass?

A

The MASS of a CHEMICAL FORMULA.

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25
Q

How are elements arranged on the periodic table?

A

In order of INCREASING ATOMIC number

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26
Q

What are the horizontal rows on the periodic table called?

A

Periods

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27
Q

What are the vertical columns on the periodic table called?

A

Groups

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28
Q

What does it mean when elements are in the same atomic group?

A

They have SIMILAR CHEMICAL PROPERTIES

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29
Q

Where are the nonmetals located on the periodic table?

A

On the right side (after staircase)

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30
Q

Where are the METALS located on the periodic table?

A

On the left side (left of staircase)

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31
Q

What is all matter made up of?

A

Atoms

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32
Q

Define an element.

A

A SUBSTANCE that contains only ONE TYPE of atom

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33
Q

What particles are found in the nucleus?

A

Protons and Neutrons

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34
Q

Where are electrons located?

A

In the electron shells

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35
Q

What is the mass of an electron?

A

0 AMU

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36
Q

What is the mass of a proton?

A

1 AMU

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37
Q

What is the mass of a neutron?

A

1 AMU

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38
Q

What is the charge of a proton?

A

+1 (Positive)

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39
Q

What is the charge of a neutron?

A

0 (Neutral)

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40
Q

What is the charge of an electron?

A

-1 (Negative)

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41
Q

What is the atomic number?

A

The number of protons in an atom.

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42
Q

What is the mass number?

A

The number of Protons + Neutrons in an atom.

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43
Q

Why do atoms have no charge?

A

Atoms have no charge because they have equal amounts of protons and electrons, which balance each other.

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44
Q

Why do elements in the same group have similar properties?

A

Elements in the same group have similar properties because they have the same number of outer electrons in their outer shell.

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45
Q

How should you write electron arrangement?

A

PAGE 6 OF DATA BOOKLET

Going from innermost shell to outermost shell, in clockwise direction.

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46
Q

What is an isotope?

A

An isotope is an atom with the same atomic number as the original element but a different mass number.

TLDR; Same atomic number, varied mass number.

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47
Q

When going down a period on the periodic table, how is reactivity affected in METALS?

A

Reactivity INCREASES as you go down a group of METALS.

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48
Q

When going down a period on the periodic table, how is reactivity affected in NON-METALS?

A

Reactivity DECREASES as you go down a group of NON-METALS.

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49
Q

What is the reactivity of the noble gases?

A

They are inert/unreactive

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50
Q

What is the top number in nucleide notation?

A

MASS number

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51
Q

What is the bottom number in nucleide notation?

A

Atomic number

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52
Q

What should nucleide notation show?

A

Atomic Number
Mass Number
Charge

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53
Q

How do you calculate RAM (relative atomic mass)?

A

RAM =
(mass of isotope A x %) + (mass of isotope B x %)
——————————————————-
100

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54
Q

What does the suffix “-ide” mean?

A

2 element compound

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55
Q

What does the suffix “-ate” mean?

A

2 Elements + Oxygen (a lot)

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56
Q

What does the suffix “-ite” mean?

A

2 Elements + Oxygen (a little)

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57
Q

What are the exceptions to the “-ide”/”-ate” rule?

A

Magnesium Hydroxide = MgH2O2
Ammonium Chloride = ClH4

58
Q

How can chemical formula be calculated?

A

SVSDF

59
Q

How do calculate formula if prefixes are involved?

A

Ignore valency

60
Q

What is a word equation?

A

An equation with the full names of each reactant and the products they form written out.

ie. Magnesium Oxide + Hydrogen –> Magnesium Hydroxide

61
Q

What does the term aqueous mean?

A

Dissolved in water

62
Q

What are roman numerals used for?

A

The valency of transition metals.

63
Q

What does a chemical formula tell you?

A

The types of atoms in a molecule and how many there are of each.

64
Q

What does the formula of a covalent network do?

A

It gives the simplest ratio of each atom in the network.

65
Q

What is an ion?

A

A charged atom

66
Q

How do you balance a chemical equation?

A

By changing the coefficients

67
Q

Define a compound.

A

Two or more atoms of DIFFERENT elements which are chemically bonded together.
(A compound is a molecule)

68
Q

What type of elements are covalent bonds between?

A

Non-metals and non-metals

69
Q

What is a covalent bond?

A

A chemical bond formed when two or more atoms share electrons.

70
Q

What holds covalent bonds together?

A

Covalent bonds are held together by two or more shared outer electrons and their attraction to the positive nuclei involved.

71
Q

What is ionic bonding?

A

Transfer of electrons

72
Q

Which elements form ionic bonds?

A

Metals and non-metals

73
Q

Do metals give or take electrons in bonding?

A

Give/lose

74
Q

Do non-metals give or take electrons?

A

Take/gain

75
Q

What type of ion do metals form?

A

POSITIVE ions (+1)

76
Q

What type of ions do non-metals make?

A

NEGATIVE ions (-1)

77
Q

What holds an ionic bond together?

A

Electrostatic attraction between the positive and negative ions

78
Q

What is a covalent network?

A

A very large structure of covalently bonded atoms.

Properties:
HIGH melting point
DOES NOT conduct electricity (excluding graphite)

79
Q

Name 5 examples of covalent networks:

A
  • Carbon (ONLY diamond and graphite)
  • Boron
  • Silicon
  • Silicon Dioxide (Quartz)
  • Silicon Carbide
80
Q

How are carbons shaped in diamonds?

A

Tetrahedral shape

81
Q

Name all of the diatomic elements.

A

BICHONF

Bromine
Iodine
Chlorine
Hydrogen
Oxygen
Nitrogen
Fluorine

82
Q

Name all molecular shapes.

A

Linear
Angular
Pyramidal
Tetrahedral

83
Q

What are intermolecular forces?

A

Intermolecular forces are the forces found in between molecules.

84
Q

Describe the intermolecular forces of a covalent molecule.

A

Intermolecular forces between a covalent network are WEAK.

85
Q

List the ways you can increase the rate of a reaction.

A
  • Increase temperature
  • Add a catalyst
  • Increase the concentration of reactant
  • Decrease in particle size/increase of surface area
86
Q

Define a catalyst.

A

A catalyst is a substance which speeds up chemical reactions, but can be recovered while CHEMICALLY UNCHANGED at the end of a reaction.

87
Q

How can you calculate the rate of reaction?

A

∆ Quantity / ∆ Time

88
Q

How would you calculate the mass of a mole of any substance?

A

Gram Formula Mass (GFM)

89
Q

How do you calculate GFM?

A

By adding up all of the RAMs inside the compound

90
Q

What is the mass of 2 moles of NaCl?

A

GFM:
•Na- 1 x 23 = 23
•Cl- 1 x 35.5 = 35.5
GFM= 23 + 35.5 = 58.5g

Sub into Formula:
n=m/GFM
2= m/58.5

Solve:
m= 2 x 58.5
m= 117g

91
Q

How can calculations be performed using the relationship between the mass and the number of moles in a substance?

A

N = m/GFM

N — Number of Moles
m — Mass
GFM — Gram Formula Mass

92
Q

How can calculations be performed using the relationship between volume, concentration and number of moles in a substance?

A

N = cv (litres)

N — Number of Moles
c — Concentration
v — Volume

93
Q

Calculate the volume of a 2 molL-1 solution containing 0.1 moles of solute

A

n=CV
V=n/C
V= 0.1/2
V=0.05L

94
Q

Calculate the mass of 500 cm3 of a 2 molL-1 solution of K2CO3

A

GFM:
• K2- 2 x 39= 78
• C- 1 x 12= 12
• O3- 3 x 16= 48
•GFM=78+12+48= 138g

Sub into Formulae:
• C=2 n=? V= 500cm3= 0.5 LITRES
• n=? m=? GFM= 138g

Solve first equation:
n=CV
n= 2 x 0.5
n= 1 mole

Use info to solve second equation:
n=m/GFM
m= n x GFM
m= 1 x 138
m= 138g

95
Q

Define solvent.

A

The SUBSTANCE that DISSOLVES the SOLUTE.

96
Q

Define solute.

A

A solute is a substance dissolved in a solvent to create a solution.

97
Q

Define solution.

A

The result of a solute dissolved in a solvent.

98
Q

What is the pH scale?

A

An indication of the hydrogen ion concentration.

Runs from 0 to 14.

<7 acid
7= neutral
>7 alkaline

99
Q

Name a feature of neutral solutions.

A

Have equal concentrations of H+(aq) and OHˉ(aq) ions.

100
Q

Name the features of acids.

A
  • HIGHER concentration of H+(aq) ions than OHˉ(aq) ions
  • <7 pH
101
Q

Describe the relationship between quantities of OHˉ ions and the periodic table.

A

As you go HIGHER in the periodic table (towards 14), the quantity of OHˉ ions INCREASES and H+ DECREASES.

102
Q

Describe the relationship between quantities of H+ ions and the periodic table.

A

As you go LOWER in the periodic table (towards 0), the quantity of H+ ions INCREASES and OHˉ(aq) DECREASES.

103
Q

Between two, what is the more common ion in ALKALIS?

A

Alkalis have a HIGHER concentration of OHˉ ions than H+ ions.

104
Q

Between two, what is the more common ion in ACIDS?

A

Acids have a HIGHER concentration of H+ ios than OHˉ ions.

105
Q

Name the features of alkalis.

A
  • Higher concentration of OHˉ ions than H+ ions
  • > 7 pH
106
Q

What is the equation for the disassociation of water?

A

H2O(l) <–> H+(aq) + OH-(aq)

107
Q

What do all acids contain?

A

Hydrogen

108
Q

What happens when you dilute an acid with water?

A
  • pH INCREASES towards 7 (water is neutral)
  • DECREASES the concentration of H+ (aq) ions.
109
Q

What happens when you dilute an alkali with water?

A
  • pH DECREASES towards 7
  • DECREASES concentration of OHˉ (aq) ions.
110
Q

What do SOLUBLE NON-METAL OXIDES form when dissolved in water?

A

ACIDIC solutions

111
Q

What do SOLUBLE METAL OXIDES form when dissolved in water?

A

ALKALINE solutions.

112
Q

State the equation for SOLUBLE METAL OXIDES dissolving in water?

A

Metal oxide + Water → Metal Hydroxide

113
Q

Define a BASE.

A

A substance that reacts with an acid to make water.

114
Q

List examples of bases.

A
  • Metal Oxides
  • Metal Hydroxides
  • Metal Carbonates
  • Ammonia
115
Q

What do SOLUBLE BASES form when dissolved in water?

A

Alkaline solutions.

116
Q

What is a neutralisation reaction?

A

A neutralisation reaction is a reaction in which a BASE reacts with an ACID to form WATER. One of the products is SALT.

117
Q

State the equation for the neutralisation reaction of metal oxide.

A

Metal oxide + Acid → Salt + Water

118
Q

State the equation for the neutralisation reaction of metal hydroxide.

A

Metal hydroxide + Acid → Salt + Water

119
Q

State the equation for the neutralisation reaction of metal carbonate.

A

Metal carbonate + Acid → Salt + Water + Carbon dioxide

120
Q

How are salts named?

A

Prefix — The NON-ACID
Suffix — The ACID NAME

121
Q

Define a SPECTATOR ION.

A

A spectator ion is an ion that is present during the reaction but remains unchanged by the reaction.

122
Q

State the neutralisation equation for magnesium reacting with hydrochloric acid.

A

Hydrochloric acid + Magnesium —> Magnesium chloride + water

HCl + Mg -> MgCl2 + H2O

123
Q

How are carbons shaped in graphite?

A

in LAYERS of HEXAGONS.

124
Q

What is the melting/boiling point of covalent networks and why?

A

Covalent networks have a very high melting and boiling point because their covalent bonds are strong and take a lot of energy to break.

125
Q

What is the melting/boiling point of covalent compounds?

A

Very low because their covalent bonds are weak.

126
Q

What is the melting/boiling point of ionic compounds?

A

Ionic compounds have a high melting and boiling point because they have strong intermolecular forces.

127
Q

What state are ionic compounds in while at room temperature?

A

Solids.

128
Q

Can covalent compounds conduct electricity?

A

No (except Graphite)

129
Q

Can covalent networks conduct electricity?

A

No (excluding Graphite).

130
Q

Can ionic compounds conduct electricity?

A

Only when in molten or aqueous state.

131
Q

What state are covalent compounds at in room temperature?

A

Any.

132
Q

Are covalent networks soluble?

A

No.

133
Q

Are ionic compounds soluble in water?

A

Most, but not all, are.

134
Q

Why can ionic compounds conduct electricity but only as aqueous or molten?

A

Molten or aqueous ionic compounds conduct electricity because the freely moving ions carry charge.

135
Q

What is the formula for sulfuric acid?

A

H2SO4

136
Q

What is the formula for nitric acid?

A

HNO3

137
Q

Define titration.

A

Titration is a method in which a solution of KNOWN CONCENTRATION is used to determine the concentration of an UNKNOWN SOLUTION.

138
Q

Metal Oxide + Acid —>

A

Salt + Water

139
Q

Metal Hydroxide + Acid —>

A

Salt + Water

140
Q

Metal Carbonate + Acid —>

A

Salt + Water + Carbon Dioxide

141
Q

How are elements arranged in the periodic table?

A

In order of increasing atomic number.

NAT5 CHEMISTRY (2 decks)

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