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Chemistry > Unit 1 - Atomic Structure > Flashcards

Unit 1 - Atomic Structure Flashcards

1
Q

What is matter made up of?

A

Atoms which can combine in different ways eg solid liquid gas

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2
Q

What are the 3 sub atomic particles

A

Protons
Neutrons
Electrons

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3
Q

What does AMU stand for

A

Atomic Mass Unit

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4
Q

What is found at the centre of the atom

A

Protons and neutrons which form a nucleus, and has electrons orbiting around it

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5
Q

What are electrons held in

A

Energy levels

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6
Q

What is meant by the atomic number and the mass number

A

Atomic number - number of protons an atom has

Mass number - number of protons AND neutrons an atom has

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7
Q

What is a protons mass, charge, and location

A

Mass - 1
Charge - +
Location - centre of nucleus

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8
Q

What is the neutrons charge, mass and location

A

Charge - 0
Mass - 1
Location - centre of nucleus

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9
Q

What is an electrons mass, charge, location

A

Mass - 1/2000
Charge - (-)
Location - orbiting round nucleus

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10
Q

What are isotopes

A

Isotopes are atoms which have the same atomic number but DIFFERENT mass number

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11
Q

What affects the rate of a reaction

A

Catalyst
Temperature
Surface area
Concentration

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12
Q

How does a catalyst affect the rate of reaction

A

As they bring reactive molecules close enough to react on the catalyst surface

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13
Q

What are the advantages and disadvantages of using a catalyst

A

Adv
Speeds up reaction
Lowers temperature of reaction

Disadv
Expensive
Potentially harmful

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14
Q

How does temperature affect the rate of reaction

A

When we heat up a reaction the particles move much faster. This means there is a greater chance of a successful collision taking place

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15
Q

How does surface area affect rate of reaction

A

The larger the surface area the greater the reaction. Large surface areas mean a greater chance of a successful collision

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16
Q

How does concentration affect rate of reaction

A

Concentration is a measure of how many solute particles are dissolved in a volume of a solvent. Increasing concentration means less space and so more chance of a successful collision

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17
Q

What is average rate

A

Average rate = change in measurement / change in time

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18
Q

How are the elements in the periodic table arranged

A

In order of increasing atomic number

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19
Q

How can we divide the elements up in the periodic table

A

Metals and non metals
Solids liquids gases
Natural and man made
Groups

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20
Q

What are the different groups in the periodic table

A 
Group 1 - alkali metals 
            2 - alkaline earth metals 
Between 2 and 3 - transition metals 
            7 - halogens 
            8 - noble gases
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21
Q

What is RAM

A

Relative Atomic Mass

Average mass of isotopes taking into account their relative proportions

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22
Q

How would you calculate the average mass

A

Cl - 2 isotopes
35. 37
Cl and Cl. 75% of Cl is 35
17. 17

(3575/100) + (3775/100)

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23
Q

What are the seven diatomic atoms

A

O2, H2, N2, F2, Cl2, Br2, I2

24
Q

What is an ion

A

When there is an imbalance in the number of protons and electrons.

25
Q

How are ions formed

A

By gaining or losing of electrons which achieves a stable electron configuration.

26
Q

What is nuclide notation

A

Used to show numbers of sub atomic particles in an atom/ion

27
Q

What is a lattice

A

A regular arrangement of ions where each positive ion is surrounded by negative ions

28
Q

What do ionic compounds have

A

High melting and boiling points as it takes a lot of energy to break the strong ionic bonds which breaks the lattice

29
Q

How else can you break down the lattice

A

Dissolving it

30
Q

When do ionic compounds only conduct electricity

A

When molten or in solution due to the breakdown of the lattice resulting in the ions being free to move

31
Q

What is a covalent bond

A

Shared pair of electrons which is attracted to the nuclei of the bonded atoms

32
Q

What leads to double or triple covalent bonds

A

Covalent bonds can be more than one bond between atoms

33
Q

What can covalent substances form

A

Discrete molecular or giant network structures

34
Q

What do covalent molecular structures have

A

Low melting and boiling points as only weak forces of attraction between molecules are being broken

35
Q

What do giant covalent networks have

A

High melting and boiling points as it takes a lot of energy to break the strong covalent network bonds

36
Q

What types of atoms make covalent bonds occur

A

Non metals, the electrons are shared between them

37
Q

What do physical properties indicate

A 
Solubility 
Conductivity 
Hardness 
State at room temp 
Appearance
38
Q

When are ionic compounds formed

A

When metal ‘ions’ and non metal ‘ions’ form ionic bonds

39
Q

What is an ion bind described as

A

Electrostatic form of attraction

Metals and non metals ions transfer electrons

40
Q

What are the common acids

A 
Sulphuric acid (H2SO4) 
Hydrochloric acid (HCl) 
Nitric acid (HNO3) 
Citric acid 
Acetic acid aka vinegar
41
Q

What do all acids contain

A

H+ ion

42
Q

What are bases made from

A

Alkalis (metal hydroxides)
Metal oxide
Metal carbonate

43
Q

What are the common bases

A 
Sodium hydroxide (NaOH) 
Copper oxide (CuO) 
Calcium carbonate (CaCO3) aka chalk
44
Q

What is neutralisation

A

When a solution has an equal amount of hydroxide ions and hydrogen ions

45
Q

What is the equation for acid and metal oxide

A

Acid + metal oxide = salt + water

46
Q

What is the equation involving acid and metal hydroxide

A

Acid + metal hydroxide (alkali) -> water + salt

47
Q

What is the equation involving acid and metal carbonate

A

Acid + metal carbonate -> salt + water + carbon dioxide

48
Q

How do you name a salt

A

The 1st part of the salts name comes from the base and the second part comes from the name of the salt

49
Q

What is an acid

A

A solution with a greater concentration of hydrogen ions than hydroxide ions

50
Q

What is an alkali

A

A solution that has a greater concentration of hydroxide ions

51
Q

What do soluble metal oxides produce when added to water

A

Metal hydroxide solutions which increase the hydroxide ion concentration

52
Q

What increases the hydrogen ion concentration

A

Soluble non metal oxides

53
Q

What are spectator ions

A

In a reaction not all substances will react. The ones that don’t are called SPECTATOR IONS. if the state symbol has changed during the reaction then the ion is NOT a spectator ion. If the state symbol HAS changed then it is a spectator ion

54
Q

What is titration

A

It is an analytical technique used to determine the accurate volumes involved in chemical reactions such as neutralisation.

55
Q

What do all substances contain?

A

Matter

56
Q

How do you know if a reaction is endothermic

A

If the temperature drops during the reaction

Chemistry (6 decks)

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