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Chemistry Mock Don't Know > Don't Know > Flashcards

Don't Know Flashcards

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1
Q

Give the formula for the maximum number of electrons in a shell

A

When n=principal quantum number

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2
Q

How do scientists know where an electron is

A

They can never be certain about the exact position of an electron but the atomic orbital shows us a 95% probability of where it is

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3
Q

Give 2 different exceptions to the general trend in ionisation energy across a period

A

Beryllium and Boron

Nitrogen and Oxygen

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4
Q

Explain why beryllium and Boron don’t follow the trend of ionisation energy increasing across a period

A

Boron has a lower first ionisation energy than beryllium. This is because beryllium’s outer electron is in a 2s sub shell, and boron’s outer electron is in a 2p sub shell. The 2p sub shell is of higher energy, and less energy is required to remove an electron from a higher energy sub shell.

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5
Q

Explain why nitrogen and Oxygen don’t follow the trend of ionisation energy increasing across a period

A

Oxygen has a lower ionisation energy than nitrogen. This is because although they both have their outer electrons in the same sub shell, in the case of nitrogen, each outer electron is in a separate 2p orbital. In contrast, in oxygen, one of the outer shells is paired up in an orbital. Pairing electrons repel each other, so less energy is required to remove this paired electron.

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6
Q

Why does the ionisation energy generally gradually increase in successive ionisation energies

A

As you remove electrons, the nuclear charge is spread between less electrons, so the remaining electrons are pulled closer to the nucleus due to a greater force being exerted on them. Therefore, the outer electron experiences a greater nuclear force, which takes more energy to overcome

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7
Q
A
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8
Q
A
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9
Q

What ion does silver form

A

Ag+

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10
Q

What ion does zinc form

A
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11
Q

What do the name of non metal ions usually end in

A

Ide

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12
Q

What is the formula for a carbonate ion

A
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13
Q

What is the formula for a nitrate ion

A
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14
Q

What’s the formula of a sulfide ion

A
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15
Q

What’s the formula for an oxide ion

A
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16
Q

What indicator would we use when titrating a weak acid with a strong base

A

Phenolphthalein

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17
Q

What indicator would we use when titrating a strong acid with a weak base

A

Methyl orange

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18
Q

Why do we only use a few drops of indicator for neutralisation reactions

A

Because indicators are weak acids, so using too much would make the result inaccurate

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19
Q

Give the steps of how to accurately measure the amount of compound we add to a solution

A

1) weigh the mass of the compound in a weighing boat
2) add the compound to the solution
3) weigh the weighing boat- take the final mass from the initial mass to get the mass added.

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20
Q

Define relative isotopic mass

A

The mass of an atom of an isotope, in comparison to 1/12th of the mass of an atom of Carbon 12

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21
Q

What is the unit for relative isotopic mass

A

It has no units

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22
Q

Define molecular formula

A

The formula showing which elements are in a molecule, and how many atoms of each element are present.

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23
Q

How do you convert from cm^3 to dm^3

A

Divide by 1000

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24
Q

How do you convert from grams per decimetre cubed to moles per decimetre cubed

A

Multiply by the relative formula mass

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25
What is room temperature
Around 20°C
26
What is room pressure
101,000 Pa
27
What is the ideal gas equation and what does every letter stand for? Include units.
pV=nRT p=Pressure (Pa) V= Volume (m^3) n=moles R= ideal gas constant (8.314 Jmol(-1)k(-1) ) T= Temperature (K)
28
29
How do you convert from °C to K
Add 273
30
How do you convert from dm³ to m³
÷1000
31
Give 4 assumptions we make with the ideal gas equation
1) the gas molecules are tiny compared to the spaces between them 2) There are no forces acting between the gas molecules 3) The gas molecules move randomly, 4) When the gas molecules collide, we assume the collisions are elastic (no net loss in kinetic energy as a result of collisions)
32
Outline how to determine the water of crystallisation of a compound by titration
33
34
What does concordant mean
Within 0.1cm³ of each other
35
Explain how Boron is an exception to the octet rule
It doesn't have enough electrons in its outer shell to achieve a noble gas configuration by covalent bonding. However, it just uses all its electrons in covalent bonds to achieve 6 electrons in its outer shell
36
Which elements can't expand their octets and why
Elements in period 1 and 2, because these elements don't have a d subshell.
37
How strong are dative bonds
They have the same strength as normal covalent bonds
38
Outline the electron pair repulsion theory
The shape of a molecule is determined by the electron pairs surrounding the central atom. This is because pairs of electrons repel all other electron pairs, so the electron pairs move as far apart as possible to minimise the repulsion
39
How strong are multiple bond covalent bonds e.g. double covalent bonds
When looking at shapes of molecules, we treat a multiple bond as a single bonding area
40
Define the term electronegativity
The ability of an atom to attract the pair of electrons in a covalent bond
41
Give 3 factors that effect electronegativity
1) the size of the positive charge in the nucleus 2) the atomic radius 3) shielding
42
What's the most electronegative element
Fluorine
43
44
Define oxidation number
A measure of the number of electrons that an atom uses to bond with atoms of other elements
45
What is the rule for oxidation number in oxygen
The oxidation state of oxygen in a compound is usually -2, however in a peroxide e.g. H202, the oxidation state of oxygen is -1
46
Give the rule for oxidation state in hydrogen
The oxidation state of hydrogen in a compound is usually +1, however in a metal hydride , the oxidation state will be -1
47
Give the rule for oxidation number in group 7 elements
Unless asked to find the oxidation state of a group 7 element, you can normally assume it will be -1
48
Give the systematic names of FeCl2 and FeCl3
FeCl2 = iron (II) chloride FeCl3 = iron (III) chloride
49
What is an oxyanion? What do their names usually end in?
A negative ion that contains the element oxygen, bonded to at least 1 other element. Their names usually end in 'ate'.
50
51
When do hydrogen bonds form
Hydrogen bonds form when hydrogen atoms covalently bond to Nitrogen, Oxygen or Fluorine
52
53
54
Give and explain 2 exceptions to the octet rule
Be and B They don't have enough unpaired electrons to reach a noble gas configuration. They pair up the upaired electrons they do have
55
What elements can expand their octet
Group 5: P, As Group 6: S, Se, Te Group 7: Cl, Br, I, At
56
Describe the structure of diamond
Each Carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral shape. The Carbon atoms are held together by strong covalent bonds.
57
Describe the structure of graphite
Each carbon atom is covalently bonded to 3 other carbon atoms in a trigonal shape. Graphite is a layered structure with delocalised electrons between the layers
58
What shape do the carbon atoms in graphene form
Hexagons
59
Define co-ordinate/dative bonding
A bond formed in the sharing of a pair of electrons when both electrons in the bond are provided by one of the bonding atoms
60
61
What shape is formed when there are 2 bonding pairs and no lone pairs? Give the name and bond angle, and draw a picture of one
Linear 180°
62
63
What is the shape formed when there are 3 bonding pairs and no lone pairs? Give the name, bond example and draw an image
Trigonal Planar 120
64
What is the shape formed when there are 4 bonding pairs and no lone pairs? Give the name, bond example and draw an image
Tetrahedral 109.5
65
What is the shape formed when there are 6 bonding pairs and no lone pairs? Give the name, bond example and draw an image
Octahedral 90°
66
What is the shape formed when there are 3 bonding pairs and 1 lone pair? Give the name, bond example and draw an image
Pyramidal 107
67
What is the shape formed when there are 2 bonding pairs and 2 lone pairs? Give the name, bond example and draw an image
Non linear 104.5
68
Outline how induced dipole-dipole forces are made
At any moment, the distribution of electrons in a molecule or atom may be uneven. This causes a temporary dipole to be present The temporary dipole induces a dipole in the neighbouring molecule. The Two molecules then attract
69
70
Where between hydrogen and N, F OR O do hydrogen bonds form
Between the H atom in one molecule and the lone pair on the electronegative atom
71
Give and explain 2 anomalous properties of water
Ice is less dense than water because it has an open lattice with the hydrogen bonds holding the bonds further apart than in the liquid state. The hydrogen bonds lengthen when the water freezes Has a higher boiling point than expected because the strong hydrogen bonds between the water molecules must be broken, and this takes more energy than expected
72
Define hydrated
A crystalline compound which contains water molecules in its structure
73
Define anhydrous
A compound left when all the water of crystallization has been removed
74
Define water of crystallization
Water molecules that form an essential part of the crystalline structure of a compound
75
Describe is the ideal gas equation
PV=nRT p=pressure (Pa) v= volume (m³) n= moles R= ideal gas constant (8.314) T=temperature (K)
76
How do you convert from cm³ to m³
×10^(-6)
77
How do you convert from °C to K
+273
78
Define dynamic equilibrium
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
79
What are the conditions used in the harbour process
Pressure=200atm Temp = 450°C Iron catalyst
80
What does a KC value of 1 tell ys
The position of equilibrium is halfway between the reactants and products
81
What does a Kc value of >1(more than 1) tell us
The position of equilibrium is more towards the products
82
What does a Kc value of <1 (less than 1) tell us
The position of equilibrium is more towards the eeactan
83
84
Give the two types of catalysts and what they are
Homogenous catalyst - in the same physical state as the reactants. Usually in the aqueous state and used between 2 solutions Heterogeneous catalyst - in a different physical state to the reactants. Reactions happen at the surface of the catalyst so increasing the surface area can further increase rate of reaction
85
Describe the physical state of the halogens
Fluorine - yellow has Chlorine - yellow-green gas Bromine- brown liquid Iodine - grey-black solid Astatine- black solid
86
Define a displacement reaction
A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of it's halide ions
87
What colour is Cl2 when dissolved in water
Pale green
88
What colour is Br2 when dissolved in water
Orange
89
What colour is I2 when dissolved in water
Brown
90
91
What colour is Cl2 when dissolved in an organic solvent
Pale green
92
What colour is Br2 when dissolved in an organic solvent
Orange
93
What colour is I2 when dissolved in an organic solvent
Purple
94
Give an advantage of adding chlorine to water
Destroys bacteria and makes water safe to drink
95
What is a disadvantage of adding chlorine to drinking water
Chlorine gas can be toxic
96
What happens the Halide ions Cl-, Br- and I- react with silver nitrate
Cl- white precipitate forms Br- Cream precipitate forms I- yellow precipitate forms
97
What happens to the precipitate from the Halide ions Cl-, Br- and I- after reacting with Silver nitrate when it reacts with Ammonia
Cl- precipitate dissolves in dilute ammonia Br- Precipitate only dissolves in concentrated ammonia I- Precipitate doesn't dissolve with ammonia
98
Define valency
The number of electrons an atom has to gain, lose or share to form a chemical bond
99
Why are group 2 known as the alkaline earth metals
They all have hydroxides that are alkaline
100
Outline and explain the physical properties of group 2 elements
1) They all have hydroxides that are alkaline, which is why group 2 elements are known as the alkaline earth metals 2) high melting and boiling points because they are held together by strong metallic bonds which take a lot of energy to break 3) good conductors of electricity because they contain delocalised electrons
101
102
Give the equation showing magnesium burning in oxygen and describe what you would see
You will see magnesium burning with a bright white flame
103
Give the equation showing calcium burning in oxygen
104
105
106
107
Define activation energy
The minimum energy required to start a reaction by the breaking of bonds
108
Define the standard enthalpy or reaction
The enthalpy change when the number of moles in the reactants as specified in the balanced chemical equation react together under standard conditions
109
Define the standard enthalpy change of formation
The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states, under standard conditions
110
Define the standard enthalpy of combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions
111
Give the formula for enthalpy change
Q=mc∆T
112
Define Hess 's law
If a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same
113
Define bond enthalpy
The enthalpy change that occurs when one mole of a given bond is broken in a molecule in the gas phase to form gaseous atoms
114
Define average bond enthalpy
The average enthalpy change that takes place when 1 mole of a given bond is broken in a molecule in the gaseous phase to form gaseous atoms
115

Chemistry Mock Don't Know (2 decks)

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