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Year 10 Science > chemistry > Flashcards

chemistry Flashcards

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1
Q

acid + metal becomes…

A

salt + hydrogen gas

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2
Q

acid + metal hydroxide becomes…

A

salt + water

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3
Q

acid + metal oxide becomes…

A

salt + water

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4
Q

acid + metal carbonate becomes…

A

salt + water + carbon dioxide

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5
Q

acid + metal hydrogen carbonate

A

salt + water + carbon dioxide

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6
Q

Strong acids

A

Will always ionise 100% of the molecules to become H+ ions

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7
Q

Weak acids

A

Ionise less than 100% of the molecules into H+ ions

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8
Q

rate of reaction equation

A
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9
Q

How to find average rate of reaction

A

Gradient between 2 points

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10
Q

How to find instantaneous rate of reaction

A

Gradient of a tangent of a point

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11
Q

Concentrated acids

A

High amount of the substance in a set volume

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12
Q

Dilute acids

A

Small amount of substance in a set volume

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13
Q

Collision theory

A

Reactant particles need to collide, when they collide, they need to:
- Be in the correct orientation
- Have enough energy (activation energy) to break apart bonds

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14
Q

Ways to change the rate of reaction

A
  • Concentration
  • Temperature
  • Surface area
  • Catalyst
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15
Q

How does increasing concentration change the rate of reaction

A
  • More particles in a given volume
  • Increases the frequency of successful collisions
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16
Q

How does increasing temperature change the rate of reaction

A
  • Increases the kinetic energy of the particles (moving around faster so have more activation energy)
  • Increases the frequency of successful collisions
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17
Q

How does increasing surface area change the rate of reaction

A
  • Increases the surface area that reactants react with
  • Increases the frequency of frequent successful collisions
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18
Q

How does adding a catalyst change the rate of reaction

A
  • Breaks/ weakens the bonds of reactants but does not get used in reaction
  • Rearranges particles to be in correct orientation
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19
Q

Catalyst definition

A

A substance that is added to speed up the rate of reaction without being a part of the chemical reaction

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20
Q

Properties of acids

A
  • Produce hydrogen ions when dissolved in water
  • Sour in taste
  • Molecular in structure
  • Dissolves substances
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21
Q

Properties of bases

A
  • Produces hydroxide ions when dissolved in water
  • Feels soapy
  • Alkaline
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22
Q

0-6 on the pH scale is…

A

Acidic

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23
Q

8-14 on the pH scale is…

A

Basic

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24
Q

Electron definition

A
  • Negative charge
  • Smaller than protons and neutrons
  • Sit in the shells of an atom
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25
Q

Protons

A
  • Have a positive charge
26
Q

Neutrons

A
  • Have a neutral charge
27
Q

Nucleus

A
  • Centre of the atom
  • Has a positive charge
  • Contains protons and neutrons
28
Q

What are ions?

A
  • A version of an atom that becomes charged through gaining or losing electrons
  • Its goal is to have a full outer shell
29
Q

Cations

A
  • Positively charged ions (more protons than electrons)
  • Mostly metals
30
Q

Anions

A
  • Negatively charged ions (more electrons than protons)
  • Mostly non-metals
31
Q

Polyatomic ions

A

OH(-): Hydroxide
CO3(2-): Carbonate
HCO3(2-): Hydrogen carbonate

32
Q

Ionic bonding

A

The bonding between a metal and a non-metal through the transfer of electrons

33
Q

Displacement reactions

A

A displacement reaction occurs when the more reactive metal is placed into a solution with a less reactive metal

34
Q

Reactivity series of elements (from most to least)

A

Potassion, Sodium, Calcium, Lithium, Magnesium, Aluminium, Zinc, Iron, Tin, Lead, Copper, Gold

35
Q

Properties of ionic compounds

A
  • Lattice structure alternating between cations and anions
  • High melting and boiling points
  • Crystalline solids
  • Conducts electricity when in molten or aqueous state
  • Hard
  • Brittle
36
Q

What is shown by the periods on the periodic table?

A
  • Horizontal rows
  • Indicate the number of shells occupied by electrons
37
Q

What is shown by the groups on the periodic table?

A
  • Vertical columns
  • Indicate the number of valence electrons that are in the atom
38
Q

Metallic bonding

A

Bonding between metals, through electrostatic attraction between delocalised electrons and metal cations.

39
Q

Properties of metallic compounds:

A
  • Good conductors of heat and electricity
  • High melting and boiling points
  • Malleable
  • Ductile
  • High density
  • Lustrous
40
Q

Covalent bonding

A
  • Occurs between 2 non-metals
  • Electrons are ‘shared’ between atoms so they have a full outer shell
  • Can join two or more elements with covalent bonding
41
Q

Atomic number

A

Indicates the number of protons (and electrons) in an atom

42
Q

Mass number

A

Indicates the number of protons and neutrons in an atom

43
Q

Types of heat treatment of metals

A
  • Annealing
  • Quenching
  • Tempering
44
Q

Annealing

A
  • Heated until red hot, called slowly
  • Large crystals with small gaps
  • Softer, more ductile
45
Q

Quenching

A
  • Heated until red hot, cooled quickly in cold water
  • Small crystals, more gaps
  • Harder but more brittle
46
Q

Tempering

A
  • Quenched, then warmed to lower temperature, cooled slowly
  • Reduces brittleness
  • Remains hard
47
Q

Law of conservation of mass

A

Atoms cannot be created or destroyed

48
Q

Why do ionic compounds have high melting and boiling points?

A
  • Large amounts of energy required to break electrostatic attraction between oppositely charged ions (strong ionic bonds)
49
Q

Why do ionic compounds have crystalline solids?

A
  • Due to their regular, repeating arrangement of ions known as an ionic lattice
50
Q

Why do ionic compounds conduct electricity when aqueous or molten?

A
  • To conduct electricity, particles muct be charged and free-moving
  • When solid, the ions are trapped in the lattice structure (not free-moving)
  • BUT in a molten or aqueous state, the positive and negative ions are free to move in a uniform way towards electricity
51
Q

Why are ionic compounds hard?

A
  • The surface of ionic compounds is not easily scratched as a strong force is needed to disrupt the ionic bonding
52
Q

Why are ionic compounds brittle?

A
  • When enough force is applied to distort the ionic lattice, ions of like charge become adjacent, repel and cause the ionic lattice to shatter
53
Q

Why are metals good conductors of electricity?

A
  • Delocalised electrons are free to move to the positive electrode
  • Are attracted due to their opposite charges
54
Q

Why are metals good conductors of heat?

A
  • Heat causes the cations and electrons to vibrate more rapidly
  • Delocalised electrons move through the lattice, passing heat on
55
Q

Why are metals malleable and ductile?

A
  • A force can push petal ions past each other as the sea of delocalised electrons holds the layers together
56
Q

Why are metals lustrous?

A
  • Delocalised electrons reflect photons of light
57
Q

Why do metals have high melting and boiling points?

A
  • Strong electrostatic bonds require large amounts of energy to break
58
Q

Why do metals have high density?

A
  • A lot of mass in a small volume
  • Cations are very close together
59
Q

Ways to extract metals

A
  • Mining
  • Roasting in air
  • Smelting
  • Electrolysis
60
Q

Electrolysis

A
  • Using electrodes to collect the metal cations on the negative terminal
61
Q

Roasting in air

A
  • Heating metal to a high temperature below melting point in the presence of air
62
Q
A

Year 10 Science (2 decks)

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