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Chemistry Test On Everything Flashcards

1
Q

What does EXOTHERMIC reactions mean

A

Temperature increase

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2
Q

What does endothermic reactions mean

A

Temperature decrease

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3
Q

What’s neutralisation include

A

Formation of a salt

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4
Q

What does effervescence reactions include

A

Gas been given off

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5
Q

Can a physical change and a chemical change be reversed

A

A physical change can be reversed but a chemical change can not be reversed

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6
Q

What are examples of a physical change

A 
Boiling water
Melting ice
Diluting juice with water 
Breaking glass
Filtering sand from water 
Separating alcohol from water by distilling
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7
Q

What are the signs of a chemical reaction

A

Colour change

Change in energy

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8
Q

What are the examples of a chemical reaction

A

Frying an egg
Toasting bread
Rust on a car
Adding sodium to water

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9
Q

What is a mixture

A

A mixture is when two or more substances are mixed together but have not actually joined together and reacted mixtures can usually be separated easily

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10
Q

How do compounds form

A

Compounds are formed when elements react together. Compounds can have different properties to the elements that make them up

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11
Q

Are compounds easy or hard to separate

A

Compounds are hard to separate into their elements

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12
Q

What does ‘ide’ mean in elements

A

If a compound has ide, it contains two types of elements

E.g. Sodium chloride - NaCl
Iron oxide - FeO

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13
Q

What does ‘ite’ and ‘ate’ mean in elements

A

If a compound ends in ‘ite’ and ‘ate’, it contains two types of element plus it also contains oxygen

E.g. Sodium chlorate - Sodium chlorine oxygen
Iron sulphate - iron sulphur oxygen

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14
Q

What’s a physical change

A

Substances may seem different, but the way the atoms link up is the same. It changes shape or size. It dissolves. It changes phase (freezes,boils,evaporation,condenses)

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15
Q

What is a chemical change

A

Changes the way the atoms link up. Makes new substances. Change in colour. Temperature change (increases or decrease). Gas given off (effervent). Formation of a solid

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16
Q

What are compounds

A

Compounds are formed when two or more elements chemically join together (bonded). The different types of atoms becomes together.

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17
Q

What is a mixture

A

Mixtures are formed when two or more different substances come together but without chemically joining. These different substances may be elements or compounds

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18
Q

What does exothermic mean

A

Heat energy given out (exit) to its surrounding (temperature increase)

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19
Q

What does endothermic mean

A

Heat energy taken it (enter) the reaction from the surroundings (temperature decrease)

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20
Q

What does diatomic mean

A

Only contains 2 atoms

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21
Q

What does solute mean

A

Solid part if the solution

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22
Q

What does solution mean

A

The combined solvent and solute

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23
Q

What does solvent mean

A

Liquid part of the solution e.g. Water

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24
Q

What does Saturated soluction mean

A

A solution where no more solute can dissolve

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25
Q

What does Aquaus mean

A

When something has dissolved in water e.g. salt water

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26
Q

What are Distillations

A

Technique used to separate a mixture of liquid using their boiling points

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27
Q

What is alloy

A

A compound of metals

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28
Q

What is filteration

A

Separation Technique used for separating a liquid and a solid

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29
Q

What are reactants

A

These are chemicals that are reacting with each other

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30
Q

What’s an independent variable

A

What is being changed

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31
Q

What’s an dependant variable

A

What you are measuring (depends if the independent or changes as a result of independence)

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32
Q

What are control variables

A

Things you keep the same so you can figure what is different
E.g. Magnesium. Copper. Zinc
0.1 acid. 0.1 acid. 0.1 acid
Mass of. Mass of Mass of
Metal Metal. Metal

You keep everything the same but change the metal

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33
Q

What is a fair test

A

Changing one thing, keeping everything else the same

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34
Q

What are enzymes

A

Enzymes are biological catalysts. They help the reactions that occur in our bodies by controlling the rate of reaction.

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35
Q

What is denature

A

Changes shape so it decrease reaction rate

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36
Q

What are catalysts

A

Substances which speed up a chemical reaction without being used up (they can be recovered)

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37
Q

What is activation energy

A

Energy required to start a reaction

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38
Q

What is homogenous catalyst

A

A catalyst in the same state as the reactions

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39
Q

What is a heterogenous catalyst

A

A catalyst in a different state as the reactants

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40
Q

What’s an isotope

A

An element which has the same protons but different neutrons

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41
Q

What are ions

A

Charged particles

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42
Q

What is a molecule

A

Two or more atoms held together by covalent bonds

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43
Q

What is a covalent bond

A

Bond between non-metals where pairs of electrons are shared

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44
Q

What is a ionic formulae

A

The ionic formula of a compound shows the charges on the ions

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45
Q

What is electricity

A

Electricity is a flow of charged particles

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46
Q

What are atoms

A

The smaller part of an element that can exist. (electron,proton,neutrons make up an atom)

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47
Q

What are some key definitions for soluble,solution,solvent

A

If something is soluble you can dissolve it to make a solution. The substance that gets dissolved is called the solute. The substance that does the dissolving is called the solvent. If something is insoluble it cannot be dissolved by the solvent

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48
Q

What are the states of matter

A

Solid - S
Liquid - L
Gas - G
Aqueaus - AQ

49
Q

What are some important notes on atoms

A

All atoms are very small particles. All the atoms in an elements are the same. Atoms make up of subatomic particles.
3 main ones - PROTON
- NEUTRON
- ELECTRON

50
Q

What are my notes on chemical reactions

A

Before a chemical reaction can take place, the particles of the reacting chemicals must collide. With a solid, only the particles on the outside can come together and react. So the larger the surface area the faster the reaction. Smaller particles means bigger surface area and so a faster rate of reactions. Larger particles means smaller surface area and a slower rate of reaction.

51
Q

How can you measure the rate of reactions

A

You can measure the rate of reaction by the mass lost. Volume of gas or temperature.

52
Q

What is activation energy

A

For the reaction to happen the particles must have a certain amount of energy - this is called activation energy

53
Q

What are the 5 things that a reaction depends on

A

1) temperature of the reactants
2) their concentration
3) their surface area
4) if a gaseous reaction - the pressure
5) whether or not a catalyst is used

54
Q

How can you speed up a reaction

A

By heating the particles - this gives them more energy

55
Q

How can you measure 1.volume of gas vs time

                                  2. Loss of mass vs time 
                                  3. Change in concentration
                                  4. Average rates and 5. 6.
A
  1. Rate = change in volume/time. 6. Volume cm3/time sec.
  2. Rate = change in mass/time
  3. Rate = change in concentration/time
  4. Rate = change in measured quality/change in time
  5. Rate = mass g/time mins
56
Q

What is the charge of protons,electrons and neutrons, where is it found and what is its mass

A

Proton - + - nucleus - 1
Electrons = - = orbiting the nucleus = 0 (or 1/17 43)
Neutrons - 0 - nucleus - 1

57
Q

What are the laws and rules of the periodic table

A

The atomic number must be smaller than the atomic mass. Protons and electrons will always be positive and negative. Electrons must add up to the same amount of protons. The amount of protons and neutrons are double the amount of electrons. No one type of atom has the same no. Protons and neutrons as another. Atomic mass=p+n

58
Q

What are isotopes

A

Isotopes are atoms of the same element with different mass numbers
That is;
Same atomic no.
Same no. of P
Different mass number
Different no. of N

59
Q

What are the isotope examples of Hydrogen

A

Protium. P-1 N-0 E-1 = used for hardening margarine
Deuterium P-1 N-1 E-1 = used in heavy or deuterated water solvent
Tritium P-1 N-2 E-1 = radioactive, used in H-bombs, glow in dark paints

60
Q

Notes on chemical bonding

A

So the most stable,most unreactive have full outer shells/energy levels. By gaining the same electron arrangement as noble gases.

61
Q

How do you form ions

A

For atoms to become ions they can either add electrons or loose electrons. To become stable s full outer energy level is needed.

62
Q

What are the 3 different types of bonding

A

Ionic binding=metal + non-metal (involves ions) (loose or gain electrons)
Metallic bonding=metal+metal (share electrons)
Covalent bonding=non-metals + non-metals (share electrons)

63
Q

What is a chemical formula.

A

A chemical formula gives the number of atoms of each element in a molecule of a colvent substance or ionic unit. Made up of symbol + numbers

64
Q

What are the steps for writing the chemical formula

A
  1. Write elements symbols MgO
  2. Write the valency at the top right hand side of each element Mg2O2
  3. Cross over the valencies
  4. Check if you can simplify the formula MgO
65
Q

What are the prefixes

A 
Mono or mon =1.            Hexa =6 
Di =2
Tri =3
Tetra =4
Penta =5
66
Q

What does it mean that opposites attract

A

The positively charged nuclei are both attracted by the shared pair of electrons

67
Q

What is ionic bonding

A

An ionic bond is frowned between a metal + non-metal

68
Q

How do you do the ionic compound formula.

A

The formula of an ionic compound is found using the valency method as covalent bonding

Valency -> cross -> divide (even if it’s y1)

69
Q

What are the symbols you use for 3D nature of molecules

A

Triangle - in front
Full line - sample place
Dotted line - behind

70
Q

What are the lines for VSEPR

A

2 bonds - linear or bent
3 bonds - pyramidal
4 bonds - tetrahedral

71
Q

What are the valencies for the groups in the periodic table metals

A

Group 1 ,1 outer electron, loses 1 electron X+
Group 2, 2 outer electrons, loses 2 electrons X2+
Group 3, 3 outer electrons, loses 3 electrons X3+

72
Q

What are the valencies for the groups in the periodic table non-metals

A

Group 5, 5 outer electrons, gains 3 electrons
Group 6, 6 outer electrons, gains 2 electrons
Group 7, 7 outer electrons, gains 1 electron

73
Q

What are the rules for the ionic formula

A
  1. Symbols
  2. Write the ion charges
  3. Balance the charges
  4. Write the ionic formulae with brackets
74
Q

What’s the name for when electrons are free to move

A

This is called delocalised

75
Q

What does electro and lysis mean

A

Electro. Lysis
⬇️. ⬇️
Using Break
Electricity Apart

76
Q

Why don’t non metals conduct

A

Non metals have no free electrons do they can’t move, so they can’t conduct electricity

77
Q

Do covalent, solid ionic compounds, aqueous ionic compounds and molten ionic compounds conduct electricity

A

Covalent compounds➡️don’t conduct➡️no charged particles
Solid ionic compounds➡️don’t conduct➡️ions can’t move
Aqueous ionic compounds➡️do conduct➡️form ions
Molten ionic compounds➡️do conduct➡️ions free to move

78
Q

What are the colours of the ions

A 
Yellow 
Orange 
Green
Colourless
Purple 
Blue
79
Q

What element is represented by yellow

A

Chromate - negative ion
Sodium chromate
Potassium chromate

80
Q

What element is represented by orange

A

Dichromate = negative ion
Potassium dichromate
Sodium dichromate

81
Q

What element is represented by green

A

Nickel = positive ion
Nickel nitrate
Nickel sulphate

82
Q

What element is represented by colourless

A

Sodium chloride
Sodium nitrate
Potassium sulphate

83
Q

What element is represented by purple

A

Permanganate = negative ion

Potassium permanganate

84
Q

What element is represented by blue

A

Copper = positive ion
Copper nitrate
Copper sulphate
Copper chloride

85
Q

What happens to the ions during ion migration

A

Positive ions. ➡️ negative electrode
(Metals/groups)

Negative ions. ➡️ positive electrode
Non-metals/groups)

86
Q

Is water ionic

A

Yes, but sometimes dissolves in ionic things

87
Q

What are the structure of ionic compounds

A

Ionic compounds have a particular structure (lattice). There are TWO types of covalent structures. Ions in a solid state cannot move, hence no conduction

88
Q

Describe ionic

A

Solid at room temperature. High melting and boiling points due to STRONG attraction between ions. Conduct electricity when molten or in solution, but NOT solid

89
Q

What’s the structure of covalent compounds (covalent discrete molecules)

A

Small molecules of a few atoms bonded together (e.g. H2O, CO2, CH4). Gas or liquid at room temperature. Low melting and boiling points due to WEAK attraction between molecules

90
Q

What’s the structure of covalent compounds (covalent networks)

A

Large networks of thousands of atoms bonded together e.g. graphite, diamond, SiO2 (sand). Solid at room temperature. High melting and boiling points due to STRONG covalent bonding between all atoms. Do NOT conduct electricity in any state (except graphite)

91
Q

Does covalent networks conduct electricity

A

Do not conduct electricity

92
Q

Does ionic lattice conduct electricity

A

Do conduct electricity when liquid but not solid

93
Q

Does metallic lattice conduct electricity

A

Conduct electricity when solid and have a wide range of melting points

94
Q

Does discrete covalent molecular conduct electricity

A

Does not conduct electricity

95
Q

What is a valency

A

The number of bonds an atoms can form (depends on group from periodic table)

96
Q

What are the rules for the chemical formula

A
  1. Write symbols of elements present in compound
  2. Put valency above each symbol
  3. Cross valency over (swap and drop)
  4. Cancel down ratio if necessary
  5. Write correct chemical formula
97
Q

What are the Roman numerals

A 
I - 1.     VI - 6 
II - 2 
III- 3 
IV- 4 
V - 5
98
Q

Why are Roman numerals used

A

Some elements, particularly the transition metals in the centre block of the periodic table can have more the one valency. Roman numerals are often used to show the valency for these elements e.g. Cu

99
Q

What are the rules for balancing equations

A
  1. Work out the number of atoms of each element on both sides of the reaction
  2. Pick an element which doesn’t balance and pencil in a number in front to make it balance
  3. Recount your atoms
  4. If your atoms still don’t balance repeat until everything balances
100
Q

What is the moles and GFM

A

In chemistry the mole is the gram formula mass (GFM) or relative atomic mass (RAM) of a substance. This is really the same as the formula mass, but with grams as the unit

101
Q

How do you do mole calculations

A

Number of moles = mass in grams ➗ mass of 1 mole
Mass (g) = number of moles ✖️mass of 1 mole
Mass of mole = mass in grams ➗ number of moles

102
Q

How do you do solution calculations

A

Number of moles (mol) = concentration ✖️ volume
Concentration (moll-1) = no. of moles ➗ volume
Volume (l) = no. of moles ➗ concentration

103
Q

Are ions present in acid and alkali solutions

A

Ions are present in acid and alkali solutions

104
Q

Why does water not conduct electricity

A

Water has a low concentration of ions. Hence acids and alkalis are far better conductors than water

105
Q

Explain what’s in a neutral solution

A

In neutral solutions such as water, the concentration of hydrogen ions H+ (AQ) and hydroxide ions OH- (AQ) is equal

106
Q

What do acids and alkalis make more of in each

A

Acids make more H+ ions in solution
Bases make more OH- ions in solution
Water contains exactly the same number of H+ and OH-

107
Q

What is neutralisation

A

Neutralisation is the reaction of an acid with a neutralised. Any substance which neutralises an acid is known as a base. Bases which dissolve in water are known as alkalis

108
Q

What are the 4 important reactions of acids

A

Acid ➕ alkali ➡️ salt and water
Acid ➕ metal oxide ➡️ salt and water
Acid ➕ metal carbonate ➡️ salt ➕ water ➕ carbon dioxide
Acid ➕ metal ➡️ sodium chloride (salt) ➕ hydrogen

109
Q

Why do we use titration

A

A bursts is an accurate way to measure the volume of a liquid as you run it into a container. In a titration we can measure exactly how much acid is needed to neutralise certain volume of alkali

110
Q

What is titration used for

A

Titration is used to find the exact concentration of a solution. Usually an acid or alkali. We measure the exact volume needed to react. Using the balanced equation for the reaction we can work out how many moles we must have. Then we use the formula conc. - moles/volume

111
Q

What are the titration calculations

A
  1. (Alkali) pvc= pvc (acid)
  2. nAlkali ✖️ c ✖️ v = nAcid ✖️ c ✖️ v
  3. C1 ✖️ V1 ➗ N1 = C1 ✖️ V1 ➗ N1
112
Q

What is the ionic equation

A

These are different to normal formula equations.

  1. Write out the normal formula equation first
  2. Any compounds that are ionic - show them as ions in which state (g,l,s)
  3. Remove any SPECTATOR IONS
113
Q

What does spectator ions mean

A

An ion that is press as both a reactant and a product in a chemical equation, spectator ions take NO PART in the reaction.

114
Q

What are reactants

A

These are the chemicals that are reacting with each other

115
Q

What happens when they react

A

Some changes may occur

116
Q

What are products

A

These are the new substances formed after the reaction

117
Q

What does molten mean

A

It described a liquid formed by melting a solid

118
Q

What is pH

A

A measure of how acidic or alkaline a substance is

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