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Chemistry > Foundations In Chemistry > Flashcards

Foundations In Chemistry Flashcards

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1
Q

What is the charge of a proton

A

1+

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2
Q

What is the charge of an electron

A

1-

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3
Q

Which particle has the same mass as a proton

A

Neutron

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4
Q

Which two particles make up most of an atoms mass

A

Protons and neutrons

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5
Q

Which letter is used to represent the atomic number of an atom

A

Z

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6
Q

What does the atomic number tell us

A

The number of protons

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7
Q

Which letter represents the mass number

A

A

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8
Q

How to calculate the number of neutrons

A

Mass number- atomic number

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9
Q

Define isotope

A

Same protons different neutrons

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10
Q

What are ions

A

Charged particles formed when an atom loses/gains electrons

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11
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared with one twelfth of the mass of an atom of carbon-12

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12
Q

Define relative isotopic mass

A

The mass of an atom of an isotope compared with one twelfth of the mass of an atom of carbon-12

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13
Q

What two assumptions are made when calculating mass number

A

Contribution of electron is ignored and the mass of both proton and neutron is taken as 1.0u

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14
Q

How to calculate relative molecular mass and relative formula mass

A

Add relative atomic masses of each atom making up the molecule or the formula

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15
Q

3 uses of mass spectroscopy

A

Identify unknown compounds
Find relative abundance of each isotope
Determine structural information

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16
Q

How does a mass spectrometer work

A

Sample made into positive ions
Pass through Apparatus and separated according to mass to charge ratio
A computer analyses the data and produces mass spectrum

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17
Q

Do metals usually gain or lose electrons

A

Lose electrons

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18
Q

What are molecular ions

A

Covalently bonded atoms that lose or gain electrons

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19
Q

Charge of an ammonium ion

A

+1

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20
Q

Charge of a hydroxide ion

A

-1

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20
Q

Charge of a hydroxide ion

A

-1

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21
Q

Charge of a nitrate ion

A

-1

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22
Q

Carbonate ion

A

-2

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23
Q

Sulfate ion

A

-2

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24
Q

Empirical formula

A

Simplest whole number ratio

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25
Q

Calculate empirical formula

A

Divide amount by molar mass
Divide by smallest number
If decimal decide by suitable number to make whole

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26
Q

Symbol for amount of substance

A

n

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27
Q

Unit to measure amount of substance

A

Mole

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28
Q

What does avogadro constant represent

A

Number of atoms per mole of carbon-12 isotope

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29
Q

Calculate mass of 1 mole of an element

A

Relative atomic mass in grams

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30
Q

Mole equation

A

Moles=mass/ molar mass

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31
Q

Avogadros law

A

Under the same temperature and pressure one mole of any gas would occupy the same volume

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32
Q

How much volume does a gas occupy at room temperature and pressure

A

24dm^3

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33
Q

Define molar gas volume

A

Volume per mole of gas molecules

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34
Q

Why do different gas particles occupy the same volume

A

Gas particles are very spread out so individuals differences have no effect

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35
Q

Moles when gas volume is given

A

Moles=volume(dm^3)/24

Moles=volume(cm^3)/24000

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36
Q

Ideal gas equation

A

Pressure(Pa)×volume(m^3) =moles×gas constant(8.314)×temperature(k)

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37
Q

0°c = how many kelvin

A

273

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38
Q

What does concentration of a solution mean

A

Amount of solute dissolved in 1dm^3 of solvent

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39
Q

Moles when given concentration and volume

A

Moles=conc×vol

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40
Q

What is a standard solution?

A

A solution of a known concentration

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41
Q

Steps to prepare a standard solution

A

Weigh solution
Dissolve solute using solvent
Pour into volumetric flask
Rinse beaker using solution and add it to flask
Add solvent until it reaches graduation line
Mix thoroughly

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42
Q

…..

A

….

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42
Q

What does percentage yield mean

A

Efficiency reactants are converted into products

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43
Q

How is percentage yeild calculated

A

Percentage yeild=actual amount of product/ theoretical amount×100

44
Q

What does atom economy mean

A

The proportion of desired products compared with all the products formed in the reaction

45
Q

How is atom economy calculated

A

Atom economy= Mr desired product/ sum of Mr of all products×100

46
Q

When an acid is added to water what in is released into solution

A

H+

47
Q

Define acid

A

Proton donor

48
Q

Describe the dissociation of a strong acid

A

Full disassociation

49
Q

Define base

A

Proton acceptor

50
Q

Which base is used to treat acid indigestion

A

Magnesium hydroxide

51
Q

What are alkalis

A

Bases that can dissolve in water to form aqueous hydroxide ion

52
Q

What are amphoteric substances

A

Substances that can act as acids and bases

53
Q

What is formed when acids react with carbonates

A

Salt carbon dioxide and water

54
Q

What is a salt

A

A compound formed when h+ of an ion is replaced by a metal ion or positive ion

55
Q

What if formed when acids react with metal oxides

A

Salt and water

56
Q

Formed when acids reacts with alkali

A

Salt and water

57
Q

Formed when acids react with metal

A

Salt and hydrogen

58
Q

How are ammonium salts formed

A

When an acids reacts with aqueous ammonia

59
Q

What are hydrated crystals

A

A crystalline structure containing water

60
Q

What does anhydrous crystals mean

A

Crystalline form that contains no water

61
Q

What does a dot formula indicate

A

The amount of water in a crystalline structure

62
Q

Method to carry out titration

A

Measure out the volume of a solution using a pipette
Add into a conical flask and add indicator
Add the other solution into a burette
Slowly add the burette solution into the conical flask
Swirl the mixture
Repeat until concordant results are obtained

63
Q

What is an oxidation number

A

The number of electrons an atom uses to bond with any other atom

64
Q

What is the oxidation number of an uncombined element

A

0

65
Q

Oxidation number of oxygen

A

-2

66
Q

Oxidation number of oxygen in peroxides

A

-1

67
Q

Oxidation number hydrogen

A

+1

68
Q

Oxidation number hydrogen( metal hydrides)

A

-1

69
Q

Oxidation number simple ion

A

The charge of the ion

70
Q

Oxidation number flourine

A

-1

71
Q

What are oxyanions

A

Negative ions that have an element along with oxygen

72
Q

Define oxidation

A

Loss of electrons
An increase in oxidation number

73
Q

Define reduction

A

Gain of electrons
A decrease in oxidation number

74
Q

What is a redox reaction

A

A reaction in which both oxidation and reduction takes place

75
Q

What does the principal quantum number indicate

A

The shell occupied by the electrons

76
Q

What is a shell

A

A group of orbitals with the same principal quantum number

77
Q

How many electrons can the 1st shell hold

A

2

78
Q

How many electron can the 2nd shell hold

A

8

79
Q

What is an orbital

A

A region around the nucleus that can hold up to two electrons with opposite spins

80
Q

When using electrons in box representation what shape is used to represent the electrons

A

Arrows

81
Q

Why does 4s orbital fill before 3d orbital

A

4s orbital has a lower energy than 3d before it is filled

82
Q

Which electrons are lost when an atom becomes a positive ion

A

Electrons in the highest energy levels

83
Q

What are the three main types of chemical bonds

A

Ionic covalent metallic

84
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions

85
Q

Define covalent bonding

A

Electrostatic attraction between a shared pair of electrons and the nuclei

86
Q

Define metallic bonding

A

Electrostatic attraction between the positive metal ions and the sea of delocalised electrons

87
Q

Electrons in which shell are represented in a dot and cross diagram

A

The outer shell

88
Q

Why does giant ionic lattices conduct electricity when liquid but not when solid

A

When solid the ions are fixed and cannot move when the are liquid they are free to move and carry a charge

89
Q

Giant ionic lattices have high or low melting and boiling point

A

High- a large amount of energy is required to overcome the electrostatic bonds

90
Q

In what type of solvents do ionic lattices dissolve

A

Polar solvents

91
Q

What is a lone pair

A

Electrons in the outer shell that are not involved in the bonding

92
Q

What is a dative covalent bond

A

A bond where both of the shared electrons are supplied by one atom

93
Q

Describe the bonding in simple molecular structures

A

Atoms within the same molecule are held by strong covalent bonds and different molecules are held together by weak intermolecular forces

94
Q

Why do simple molecular structures have low melting and boiling points?

A

Small amount of energy is enough to overcome the intermolecular forces

95
Q

Can simple molecular structures conduct electricity

A

No

96
Q

Properties of giant covalent structures

A

High melting and boiling points
Non conducters of electricity
Insoluble in polar and non polar solvents

97
Q

What is the shape and bond angle- 2 bonded pairs and 0 lone pairs

A

Linear 180°

98
Q

3 bonded pairs 0 lone pairs

A

Trigonal planar 120°

99
Q

4bonded pairs 0 lone pairs

A

Tetrahedral 109.5°

100
Q

5 bonded pairs 0 lone pairs

A

Trigonal bipyramid 90° and 120°

101
Q

6 bonded pairs and 0 lone pairs

A

Octahedral 90°

102
Q

3 bonded pairs 1 lone pair

A

Pyramidal 107°

103
Q

2 bonded pairs 2 lone pairs

A

Non linear 104.5°

104
Q

Define electronegativity

A

The ability of an atom to attract the pair of electrons in a covalent bond

105
Q

What are the two types of intermolecular forces

A

Hydrogen bonding
Van der waal’s forces

106
Q

What are the 2 interactions that can be referred to as van der waal’s forces

A

Induced dipole-permanent dipole
Permanent dipole- permanent dipole

107
Q

Describe London forces

A

London forces are caused by random movements of electrons
Leads to instantaneous dipoles
These induce a dipole in nearby molecules
These attract each other

108
Q

Does boiling point increase or decrease down the noble gas group

A

Increases no. Electrons increases hence the strength of London forces also increases

Chemistry (3 decks)

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