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National 5: Chemistry > Unit 1: Chemical Changes and Structure > Flashcards

Unit 1: Chemical Changes and Structure Flashcards

1
Q

What affects the Rate of Reaction?

A

Concentration

Particle Size

Temperature

Use of a Catalyst

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2
Q

How do you measure the rate of reaction?

A

Measuring:

  • Changes in Mass(At Regular Time Intervals)
  • Changes in Volume (At Regular Time Intervals)
  • Changes inConcentration (At Regular Time Intervals)
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3
Q

What are reactions caused by?

A

Particles colliding with each other

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4
Q

Why does High Temperature affect Reaction Rate?

A

Particles have more energy and move quicker causing more frequent collisions with more energy

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5
Q

Why does Small Particle Size affect Reaction Rate?

A

Increased surface area means a higher chance of particles colliding

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6
Q

Why does High Concentration affect Reaction Rate?

A

More particles moving means more particle collisions

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7
Q

Calculating Rate of Reaction

A

Average Rate = Change in measurable Quantity/Change in Time

Units depend on measurable quantity and time

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8
Q

Reaction Graphs

A

Steeper Gradient = Faster Reaction

Flat/Straight line = End of Reaction

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9
Q

Atoms

A

Particles that make up everything. Made from protons, neutrons and electrons

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10
Q

Electrons

A

Negatively charged particles that orbit the nucleus. Their mass is so small it is nearly 0

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11
Q

Protons

A

Positively charged particles contained in the nucleus of the atom. Have a mass of 1amu

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12
Q

Neutrons

A

Particled with no charge that are also contained in the nucleus. Have a mass of 1amu

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13
Q

Nucleus

A

Centre of an atom made up from protons and neutrons. Has an overall positivie charge

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14
Q

Group 1

A

Alkali Metals. React rapidly with water, producing an alkaline solution and hydrogen gas

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15
Q

Group 0/8

A

Noble Gases. Very unreactive and exist as individual atoms

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16
Q

Atomic Number

A

How many protons an element has

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17
Q

Mass Number

A

Number of protons and neutrons in an atom

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18
Q

Isotopes

A

Atoms with the same atomic number but different mass numbers

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19
Q

Relative Atomic Mass (RAM)

A

Calclated from the masses of all the isotopes of an element taking into account the percentage proportion of each

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20
Q

Covalent Bond

A

A shared pair of electrons between two non-metal atoms

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21
Q

Diatomic Molecules

A

Bromine

Iodine

Chlorine

Fluorine

Oxygen

Hydrogen

Nitrogen

22
Q

Linear Molecule

A

One shared electron

23
Q

Bent Molecule

A

Two shared Electrons

24
Q

Pyramidal Molecule

A

Three Shared Electrons

25
Q

Tetrahedral Molecule

A

Four Shared Electrons

26
Q

Ionic Bonding

A

Formed between a metal and a non-metal. An electrostatic force of attraction between a charged metal ion and an oppositely charged non-metal ion

27
Q

Ionic Compunds

A

Easily Dissolve in water to form a conductive solution

Very high melting points

Don’t conduct when solid

Solid at room temperature

28
Q

Covalent Network

A

Very high melting/boiling point

Solid at room temperature

Don’t conduct (except graphite)

29
Q

Electrolysis

A

The breaking up of an ionic compund using electricity. Charged particles attracted to oppositely charged electrode where they lose/gain electrons to become neutral atoms/molecules

30
Q

Prefixes

A

Mono - 1

Di - 2

Tri - 3

Tetra - 4

Penta - 5

Hexa - 6

31
Q

Balanced Equations

A

When there are the same number of the type of every atom on both sides of the equation

32
Q

Mass of One Mole

A

Gram Formula Mass (GFM)

33
Q

Mole Calculations

A

Mass(g) = Number of Moles x Gram Formula Mass

m = n x GFM

34
Q

Concentration Calculation

A

Number of Moles = Concentration (mol l-1) x Volume (l)

n=cv

35
Q

Acids pH

A

Less than 7

36
Q

Alkalis pH

A

More than 7

37
Q

Neutral/Water pH

38
Q

Formin Alkalis

A

Metal Oxide (base) dissolved in Water

39
Q

Forming Acids

A

Non-Metal Oxide Dissolved in Water

40
Q

When do Acids Occur?

A

When there are more H+ ions than OH- ions

41
Q

When do Alkalis Occur?

A

There are more OH- ions than H+ ions

42
Q

When do Neutral Solutions Occur?

A

There are an equal number of OH- ions and H+ ions

43
Q

Dilution

A

Moving an acid or alkalis pH towards 7 with water.

Occurs as there is a lower concentration of ions as water is added

44
Q

Neutralisation

A

Reaction of an acid with a base that results in the pH moving towards 7

45
Q

Neutralisation Equations

A

Acid + Alkali → Salt + Water

Acid + Metal Oxide → Salt + Water

46
Q

Neutralisation with Carbonates

A

H+ ion reacts with CO32- to form water and carbon dioxide

47
Q

Metal Carbonate Neutralisation Equation

A

Metal Carbonate + Acid → Salt + Water + Carbon Dioxide

48
Q

Carbon Dioxide Test

A

Tuns lime water milky/chalky white

49
Q

Formation of Water

A

Hydrogen ion and Hydroxide ion combine to form water

H+(aq) + OH-(aq) → H2O(l)

50
Q

Titration

A

Used to find the concentration of an Acid/Alkali

51
Q

Base

A

Substance that reacts with an acid forming water

National 5: Chemistry (3 decks)

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