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Chemistry Y10 > end of year revision Y10-Chemistry > Flashcards

end of year revision Y10-Chemistry Flashcards

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1
Q

The random movement of particles from an area of high concentration to an area of low concentration

A

diffusion

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2
Q

the conversion of solid to gas is called ——— and the reverse process is usually called——–

A

the conversion of solid to gas is called sublimation and the reverse process is usually called deposition

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3
Q

compare the state of matter in terms of

arrangement of particles

movement of particles

closeness of particles

A
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4
Q

Solids, liquids and gases have different physical properties. Why?

A

The difference in these properties comes from differences in how the particles are arranged in each state.

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5
Q

When matter changes from one state to another due to changes in temperature or pressure, the change is called an ————————

A

When matter changes from one state to another due to changes in temperature or pressure, the change is called an interconversion of state

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6
Q

in the diffusion of red-brown bromine gas experiment

After 5 minutes we see the bromine gas has diffused from the bottom jar to the top jar. explain why

A

Explanation:

The air and bromine particles are moving randomly and there are large gaps between particles

The particles can therefore easily mix together

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7
Q

fill in the table

A
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8
Q

Solubility is ————

A

Solubility is a measurement of how much of a substance will dissolve in a given volume of a liquid

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9
Q

The solubility of a gas depends on —————-and ————–

As pressure —————-, gases become more soluble

As temperature ————-, gases become less soluble

A

The solubility of a gas depends on pressure and temperature

As pressure increases, gases become more soluble

As temperature increases, gases become less soluble

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10
Q

Solubility of solids is affected by —————

A

Solubility of solids is affected by temperature

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11
Q

If at 40 °C the solubility of potassium nitrate is 68 g per 100 g of water

Determine how much potassium nitrate will dissolve in 20 g of water at 40 °C?

A

68 x (20 / 100) = 13.6 g of potassium nitrate will dissolve in 20 g of water

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12
Q

plotting a diagram

Graph:

Use the results to plot a solubility curve for ammonium chloride at different temperatures. Solubility is on the y-axis and temperature is on the x-axisConclusion:

The shape of the graph will allow to state how the solubility varies with temperature

A
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13
Q

to calculate the solubility of a solute in 100g of water ( solvent)

= mas of solute/mass of solvent x100

A

solubility (g.100g of water is

= mas of solute/mass of solvent x100

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14
Q

Melting and boiling points data can therefore be used to distinguish pure substances from mixtures

explain why

A

because

Pure substances melt and boil at specific and sharp temperatures while

mixtures have a range of melting and boiling points as they consist of different substances .

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15
Q

used to separate a liquid and soluble solid

A

simple distillation

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16
Q

used to separate two or more liquids that are miscible with one another (e.g., ethanol and water from a mixture of the two)

A

Fractional Distillation

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17
Q

Used to separate an undissolved solid from a mixture of the solid and a liquid / solution ( e.g., sand from a mixture of sand and water)

A

Filtration

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18
Q

Used to separate a dissolved solid from a solution, when the solid is much more soluble in hot solvent than in cold (e.g., copper sulphate from a solution of copper (II) sulphate in water)

A

Crystallisation

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19
Q

used to separate substances that have different solubilities in a given solvent (e.g., different coloured inks that have been mixed to make black ink)

A

Paper Chromatography

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20
Q

Rf = distance travelled by substance ÷ distance travelled by solvent

A
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21
Q

define the term atom

A

the smallest piece if an element that can still be recognised as that element

it surrounds the nucleus that includes protons and neutrons

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22
Q

define the term molecule

A

a group of two or more atoms chemically bonded together

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23
Q
A

Note

Isotopes are easy to recognize from their notation as they have the same symbol but different mass numbers. For example, the two stable isotopes of copper are 63Cu and 65Cu

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24
Q

answer the question

A
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25
Q

Why atoms react with other atoms ?

A

atoms react with other atoms in order to achieve a full outer shell of electrons (which would make them more stable)

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26
Q

The arrangement of electrons into shells for an atom (e.g. electronic configuration of carbon is 2 . 4)

A

Electronic configuration

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27
Q

identify properties of metals non-metals

A
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28
Q

Why Noble Gases (group 0) are Unreactive?

A

The elements in group 0 of the periodic table are called the noble gases

They are all non-metal, monatomic (exist as single atoms), colourless, non-flammable gases at room temperature

The group 0 elements all have full outer shells of electrons, they do no need to participate in reactions to complete their outer shells by losing, gaining, or sharing electrons.

therefore they are unreactive and extremely stable

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29
Q

balance the equation

1.___P4 + ___O2 à ___P2O5

also refer to sheet 0

A

1.___P4 + _5_O2 à _2_P2O5

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30
Q

calculate formula mass and percentage composition

(NH4)2SO4

refer also to sheet 1

A

Formula unit mass for (NH4​)2​SO4​
=2×atomic mass of N+8×atomic mass of H+1×atomic mass of S

+4×atomic mass of O
=2×14+8×1+1×32+4×16
=28+8+32+64
=132

132 g/mol

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31
Q

How many moles are in 2.64 g of sucrose, C12H22O11 (Mr = 342.3)

A

The molar mass of sucrose is 342.3 g mol-1

The number of moles is found by mass ÷ molar mass

This comes to 2.64 g ÷ 342.3 g mol-1 = 7.71 x 10-3 mol

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32
Q

What is the mass of 0.250 moles of zinc?

also refer to sheet 2

and remember the triangle

A

Answer:

From the periodic table the relative atomic mass of Zn is 65.38

So, the molar mass is 65.38 g mol-1

The mass is calculated by moles x molar mass

This comes to 0.250 mol x 65.38 g mol-1 = 16.3 g

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33
Q

Calculate the mass of magnesium oxide that can be made by completely burning 6.0 g of magnesium in oxygen in the following reaction:

2Mg (s) + O2 (g) ⟶ 2 MgO (s)

also refer to Sheet 3

A
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34
Q

Calculate the mass of aluminium, in tonnes, that can be produced from 51 tonnes of aluminium oxide. The equation for the reaction is:

2Al2O3 ⟶ 4Al + 3O2

A
35
Q

Copper(II) sulfate may be prepared by the reaction of dilute sulfuric acid on copper(II) oxide. A student prepared 1.6 g of dry copper(II) sulfate crystals. Calculate the percentage yield if the theoretical yield is 2.0 g.

also refer to sheet 4

A

Actual yield of copper(II) sulfate = 1.6 g

Percentage yield of copper(II) sulfate = (1.6 / 2.0) x 100

Percentage yield = 80%

36
Q

limiting reagents

please refer to sheet 5

A
37
Q

The empirical formula of X is C4H10S1 and the relative formula mass of X is 180. What is the molecular formula of X?Relative atomic masses: carbon : 12 hydrogen : 1 sulfur : 32

also refer to sheet 6

A

Step 1 - Calculate the relative formula mass of the empirical formula

(C x 4) + (H x 10) + (S x 1) = (12 x 4) + (1 x 10) + (32 x 1) = 90

Step 2 - Divide the relative formula mass of X by the mass of the empirical formula

180 / 90 = 2

Step 3 - Multiply each number of elements by 2

(C4 x 2) + (H10 x 2) + (S1 x 2) = (C8) + (H20) + (S2)

Molecular Formula of X = C8H20S2

38
Q

define the term empirical formula

A

gives the simplest whole number ratio of the atoms present in a compund. It can be worked out from experimental data

39
Q

a form of energy a substance possesses due to motion

A

kinetic energy

40
Q

—————–refers to the amount of solute there is in a specific volume of the solvent

A

Concentration

41
Q

Example 1Calculate the amount of solute, in moles, present in 2.5 dm3 of a solution whose concentration is 0.2 mol dm-3.

also refer to sheet 7

A
42
Q

define the term titration

A

a technique used to follow the course of a neutralisation reaction between an acid and an alkali. it can be used to find out how much of an acid/alkali reacts with a certain volume of an alkali/acid

43
Q

How to carry out a titration

A

Method:

Use the pipette and pipette filler and place exactly 25 cm3 sodium hydroxide solution into the conical flask

Place the conical flask on a white tile so the tip of the burette is inside the flask

Add a few drops of a suitable indicator to the solution in the conical flask

Perform a rough titration by taking the burette reading and running in the solution in 1 – 3 cm3 portions, while swirling the flask vigorously

Quickly close the tap when the end-point is reached (sharp colour change) and record the volume, placing your eye level with the meniscus

Now repeat the titration with a fresh batch of sodium hydroxide

As the rough end-point volume is approached, add the solution from the burette one drop at a time until the indicator just changes colour

Record the volume to the nearest 0.05 cm3

Repeat until you achieve two concordant results (two results that are within 0.1 cm3 of each other) to increase accuracy

44
Q

crystalization

Example: 49.9g of hydrated copper sulphate is heated, and produces 31.9g of the anhydrous copper sulphate.
What is the formula of the hydrated crystal?

A

31.9 g of CuSO4 RFM 63.5 + 32 + (4x16) = 159.5 g/mol

Moles of anhydrous = 31.9/159.5 = 0.2 moles

So, moles of hydrated crystal must have been = 0.2 moles

Using formula triangle?

Mr of hydrated crystal

= mass/moles = 49.9/0.2 = 249.5g/mol

What is the total mass of the waters of

crystallisation?

249.5 - 159.5

= 90 g/mole

So, moles of water =90/18 = 5

So formula of the hydrated crystal is CuSO4.5H2O

45
Q

•What volume oxygen is needed to react with 14g of H2 in the following reaction?

A
  • 2H2 + O2 → 2H2O
  • Moles of H2 = 14/2 = 7 moles.

•

•Moles of O2 = 7/2 (from 2: 1 ratio) 3.5 moles.

•

  • Volume of O2?
  • 3.5 x 24dm3 = 84dm3
46
Q

•What volume carbon dioxide is produced when 36g of methane is combusted?

also refer to sheet 8

A
  • CH4 + 2O2 → CO2 + 2H2O
  • Moles of CH4 (Mr =16)
  • 36/16 = 2.25 moles

•

•Moles of CO2 = 2.25 moles (1:1 ratio in the equation)

•

  • Volume of CO2?
  • 2.25 x 24 = 54dm3
  • Volume of O2needed?
  • 1: 2 ratio fromCH4 = 4.5 moles

2:1 ratio from CO2 volume! 108dm3

47
Q

go to exam style sheet before moving to next topic

good luck

A
48
Q

The Charges of Common Positive Ions Tabl

A
49
Q

The Charges of Common Negative Ions Table

A
50
Q

what is the formula of aluminium sulfate?

use swap method

A

Write out the formulae of each ion, including their charges

Al3+ SO42-

Balance the charges by multiplying them out:

Al3+ x 2 = +6 and SO42- x 3 = -6; so +6 – 6 = 0

So the formula is Al2(SO4)3

51
Q

define the term ionic bonding

A

strong electrostatic force of attraction between oppositly charged ions formed by the transfer of electrones from one atom to another

52
Q

define the term ion

A

charged particle formed when an atom loses or gains electrones

53
Q

properties of ionic substances

A
54
Q

what is giant ionic lattice?

A

the arrangement of ions in an ionic compound in its solid state

55
Q

draw a cross dot diagram of

MgO

A
56
Q

define the term intermolecular force

A

force of attraction betwwen covalent molecules much weaker than covalent bonds within the molecules

57
Q

Covalent bonds between atoms are very strong

true or false

A

true

58
Q

define the term convalent bonding

A

trong electrostatic force of attraction between the nuclei of the atoms making up the bond and the shared pair of electrons

59
Q

•Draw dot and cross diagrams of

•

•H2 Br2 NH3 HCl H 2S

•

•Then draw the molecular structure of these molecules

A
60
Q

why is the covalent bond strong?

A

because the shared pair of electrons is attracted to the nucleus of both atoms forming a strong bond

61
Q

why chlorine is a gas at room temperature?

A

because of the weak intermolecular forces between mulecules that doesn’t take much energy to break

62
Q

substances made of covalent molecules have low melting point

explain why

A

They have low melting and boiling points as they have weak intermolecular forces acting between the molecules that doesn’t take much energy to break

63
Q
A
64
Q

What is a molecule?

A

What is a molecule?•A group of atoms held together by covalent bonds

65
Q

What is a covalent bond?

A
  • A shared pair of electrons
  • (Attracted to the nucleus of both atoms).
66
Q

covalent compounds do not conduct electricity, why?

A

covalent bonds have no ions, and no mobile electrons,

67
Q

draw

C6H6

A
68
Q

•Giant covalent structures, are insoluble explain why

A

because giant structue has no small molecules or ions that can be seperated by solvent molecules

69
Q

diamond is veyr hard where graphite is soft

A

diamond has a giant covalent structure held together by strong covalent bonds

graphite has layers that are held together by delocalised electrones , layers can slide over each other making it easy to be flaked off

70
Q

diamond melting point is high

A

has a giant structure held together by stron covalent bond that require a lot of energy to break it

71
Q

•Explain why CO2 is a gas at room temperature, yet SiO2 is a solid

A

SiO2

  1. Giant covalent structure
  2. Held together by Strong covalent bonds
  3. Lots of energy required to break them.

CO2

  1. Simple molecular covalent
  2. Weak intermolecular forces
  3. Not much energy required to break them.
72
Q

graphite can conduct electricity explan why

A

it has layers and between layers has delocalized electrones that can move and conduct electricity

73
Q
A
74
Q

C60 fullerene molecule is a simple molecular structure and has intermolecular forces

A

true

75
Q

In this fullerene, 60 carbon atoms are joined together forming 20 hexagons and 12 pentagons

A

true

76
Q

why compounds with giant ionic lattices have high melting and boiling points

A

Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions. These compounds have high melting points and high boiling points because of the large amounts of energy needed to break the many strong bonds.

77
Q

define intermolecular forces term

A

forces between molecules

78
Q

ionic bond lattice structure

A
79
Q

metallic bond lattice structure

A
80
Q

define metallic bond

A

is the electrostatic attraction between the lattice of positive metal ions and the sea of delocalised electrons”

81
Q
A
82
Q

metallic properties

A
83
Q

Why are ionic solids brittle?

A

When layers slide past each other in an ionic substance.

The like-charged ions are forced next to each other.

The ions repel.

The ionic bonding is disrupted.

84
Q

Covalent compounds do not undergo electrolysis why?

A

Covalent compounds cannot conduct electricity hence they do not undergo electrolysis

Chemistry Y10 (5 decks)

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