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Exam revision semester 1 > chemistry exam revision > Flashcards

chemistry exam revision Flashcards

1
Q

what is an atomic number?

A

the number of protons in an element and also the number of electrons in a neutral atom of an element.

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2
Q

what is an atomic mass (mass number)

A

the number of protons + neutrons in an isotope of an element

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3
Q

what 3 things need to happen for a reaction to occur? ( collision theory)

A
  1. particles must collide
  2. particles must have enough energy
  3. particles must hit at correct orientation
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4
Q

what factors increase the reaction rate?

A
  1. increasing temp
  2. increasing concentration of reactants
  3. increasing the surface area
  4. adding a catalyst
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5
Q

which has a higher surface area? a whole tablet or a crushed tablet

A

crushed tablet

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6
Q

How does increasing the temperature increase the reaction rate?

A

Increasing the temperature provides particles will kinetic energy. This makes particles move more/faster and collide more frequently.

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7
Q

How does increasing the concentration increase the reaction rate?

A

The more concentrated a substance the more particles there are in the same volume of space.-This clumps the particles together closer, leading more more frequent collisions.

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8
Q

How does increasing the surface area increase the reaction rate?

A

Increasing the surface area, increases the number of particles exposed to the reactants.More particles, leads to more frequent collisions.

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9
Q

How does a catalyst increase reaction rate?

A

-catalyst is not involved in the reaction-A catalyst decreases the activation energy/energy require for a reaction to occur.

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10
Q

On the periodic table, which number is the atomic number? big or small.

A

small

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11
Q

On the periodic table, what is the large number referred to as?On the periodic table, what is the large number referred to as?

A

atomic mass

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12
Q

The atomic number indicates the number of what in an atom?

A

protons

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13
Q

The atomic mass indicates the number of what in an atom?

A

the SUM of protons and neutrons in the atom

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14
Q

What 3 things make up an atom?

A

protons, neutrons and electron

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15
Q

what charge are electrons?

A

negative

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16
Q

What charge are neurtons?

A

neutral

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17
Q

what particles are in the atom’s nucleus?

A

protons and neutrons

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18
Q

How many electrons can be in each electron shell?

A

1st= max 2
2nd = max 8
3rd= max 8
4th = max 18

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19
Q

what is a valance electron?

A

The electrons that are in the outermost shell

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20
Q

How can the periodic table tell us the number of valence electrons an atom has?

A

the period groups.

group 4= 4 valence electrons
group 13= 3 valence electrons

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21
Q

Which side of the period table are most metals located

A

middle and left hand side

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22
Q

what side of the periodic table are most non-mentals found

A

the right hand side

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23
Q

what is the name given to group 1 metals?

A

Alkali mentals

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24
Q

what is the name given to group 2 metals?

A

Alkaline metals

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25
Q

what is the name given to group 17 metals?

A

halogen

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26
Q

what is the name given to group 18 mentals

A

Nobel gases

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27
Q

What is an isotope?

A

A variation of the same atom with different numbers of neutrons

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28
Q

The atomic size of atoms increases in what direction across the periodic table?

A

-From right to left
- & from top to bottom

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29
Q

The reactivity of metals increases as you go…
up or down the periodic table?

A

down

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30
Q

BOTH
Why does the atomic size of atoms increase as you more left across and down the periodic table?

A

Because the number of charged particles in the nucleus decreases (protons). This creates less electrostatic attraction between protons and the electrons. This means that electrons will NOT get pulled closer to the nucleus, but rather stay further away. This creates a larger atomic size.

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31
Q

BOTH
Why does the reactivity of metals increase as you move down the periodic table?

A

Because there is less electrostatic attraction between the protons and the electrons. Therefore, the electrons are more easily pulled away from the atom to react.

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32
Q

The reactivity of metals increases as you go…left or right across the periodic table?

A

from right to the left

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33
Q

Are the reactivity trends of non-metals the same or opposite to metals?

A

opposite

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34
Q

What is an ion?

A

A charged atom.
An atoms that has lost or gained electrons

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35
Q

If an atom loses an electron will it be positively or negatively charged?

A

positive

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36
Q

If an atom gains an electron will it be positively or negatively charged?

A

negatively

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37
Q

If an atom gains 3 electrons what will its valence/charge be?

A

3-

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38
Q

The periods that run across the periodic table tell you what about an atom?

A

The number of orbital energies it has.
Lithium is in period 2 and will have 2 shells of electrons.

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39
Q

What are some characteristics of alkali metals?

A

-VERY soft
-VERY reactive
-have 1 valence electron

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40
Q

What are some characteristics of alkine metals?

A

-soft
-reactive
-have 2 valence electron

41
Q

What are some characteristics of metalloids?

A

have characteristics of metals and non-metals

42
Q

What type of elements are involved in metallic bonding?

A

metals only

43
Q

What type of elements are involved in ionic bonding?

A

metals and non- metals

44
Q

What type of elements are involved in covalent bonding?

A

non-metals only

45
Q

What are some characteristics of metallic substances?

A

shiny/lustrous
-malleable
-good conductors of heat and electricity
-ductile
- high melting point

46
Q

What are some characteristics of ionic substances?

A

-very brittle (form a lattice)
-bad conductors in solid state
-good conductors in aqueous state
-strong
-high melting point

47
Q

What are some characteristics of covalent substances?

A

-bad conductors
-good insulators
-brittle
-low boiling point

48
Q

Why are metals good conductors?

A

-because they have free floating delocalised electrons that are charged and can carry heat or an electrical current through them easily.

49
Q

Why are ionic substances brittle?

A

Because they are in the form of a lattice.
-When they are hit/impacted it will cause two like charges to align.
-when 2 like charges align they will repel each other and break the substance/lattice.

50
Q

Why are ionic substances conductors in an aqueous solution and not as a solid?

A

because as a solid all the particles are locked into a lattice. Therefore, there are not free moving charged particles available to carry heat or a current.
-When in an aqueous solution the ionic substance dissociates into ions. These ions have charges. These charged particles are free to move and carry heat or a current.

51
Q

Why are ionic substances conductors in an aqueous solution and not as a solid?

A

because as a solid all the particles are locked into a lattice. Therefore, there are not free moving charged particles available to carry heat or a current.
-When in an aqueous solution the ionic substance dissociates into ions. These ions have charges. These charged particles are free to move and carry heat or a current.

52
Q

What happens to electrons in ionic bonding?

A

-they are transferred.
-the metal loses electrons
-the non-metal gains electrons

53
Q

What happens to electrons in covalent bonding?

A

-the non-metals share electrons

54
Q

What happens to electrons in metallic bonding?

A

-the metals shared electrons in a sea of delocalized electrons

55
Q

Are brackets needed when writing chemical/ionic formula with NO polyatomic molecules?

A

no

56
Q

Are brackets needed when writing chemical/ionic formula with ONE polyatomic molecules?

A

no

57
Q

what is a subscript

A

a small number on the bottom right of an element

58
Q

what does a subscript tell us

A

how many of those atoms are in the compound/molecule/element

59
Q

what is a coefficient

A

A large number at the front of a compound/molecule/element that indicates how many of that compound/molecule/element there are.

60
Q

Is chloride a polyatomic atom?

A

no

61
Q

Is nitrate a polyatomic atom?

A

yes

62
Q

Is hydroxide a polyatomic atom?

A

yes

63
Q

Is Aluminium a polyatomic atom?

A

no

64
Q

Is phosphate a polyatomic atom?

A

yes

65
Q

If an element is not in a compound/molecule, how do you write it’s chemical formula?

A

-Just write the element.

Calcium = Ca

66
Q

What are diatomic elements?

A

-elements that naturally exist in pairs.

67
Q

What elements are diatomic?

A

oxygen
fluorine
nitrogen
hydrogen
chlorine

68
Q

How many electrons do atoms want to be stable?

A

8

69
Q

when naming compounds… what three letters do you end in?

A

“ide”

70
Q

If naming an ionic compound, do you need to write prefix (mono,di, tri)?

A

no

71
Q

if naming a covalent compound, do you need to write prefix (mono,di,tri)?

A

yes

72
Q

If you have only 1 of the first element in a covalent compound.. do you need to write mono?

A

no

73
Q

What are reactants?

A

substances that start a reaction

74
Q

What are products?

A

substances that are produced from a reaction

75
Q

What is the law of conservation of matter?

A

matter cannot be created or destroyed

76
Q

What is the chemical formula for hydrochloric acid?

A

HCI

77
Q

What is the chemical formula for sulfuric acid?

A

H2SO4

78
Q

What is the chemical formula for Phosphoric acid?

A

H3PO4

79
Q

What is the chemical formula for Nitric acid?

A

NHO3

80
Q

In a precipitation reaction/ionic reaction. Do you write all the compounds present or only the ions that make the precipitate?

A

only the ions that make the precipitate

81
Q

What is a precipitate?

A

an insoluble solid that is formed when two solutions are mixed?

82
Q

what does soluble mean?

A

A substance can dissolve

83
Q

what does insoluble mean?

A

a substance that cannot dissolve

84
Q

what is solute

A

the substance that is dissolving.
Eg. salt.

Salt dissolves in water

85
Q

what is solvent?

A

the substance that something dissolves in.
Eg. water

water dissolves salt

86
Q

what does concentrated mean?

A

There are lots of particles within the volume of space.

87
Q

what does dilute mean?

A

there are very few particles within the volume of space.

88
Q

When writing the chemical/ionic formula for a substance… what is the aim?

A

balancing the charges and cancelling them out!

89
Q

What symbol is used to show a chemical reaction in an equation?

A

an arrow

90
Q

BOTH
Count the atoms in the following atoms:

C6H12O6

A

Carbon= 6
Hydrogen= 12
Oxygen =6

91
Q

How do you show an aqueous solution in an equation?

A

(aq)

92
Q

How can you identify the precipitate in a reaction?

A

Identify the insoluble product from the reaction using the solubility table

93
Q

In a precipitation reaction between substance AB and substance CD, what are the products?

A

AD and CB

94
Q

Do you look for a precipitate in the reactants or the products of an equation.

A

products only !

95
Q

In an ionic dot diagram, do you need to draw brackets?

A

yes

96
Q

In a covalent dot diagram, do you need to draw brackets?

A

no

97
Q

In ionic and covalent dot diagrams do you need to draw all electrons or just the valence electrons?

A

just the valance electrons

98
Q

If an atom has a charge of 3+, how many electrons has it gained or lost?

A

lost 3

Exam revision semester 1 (4 decks)

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