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Science > C1- Atomic structure and the periodic table > Flashcards

C1- Atomic structure and the periodic table Flashcards

1
Q

Define isotope

A

Different forms of the same element which have the same number of protons but a different number of neutrons.

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2
Q

Define element

A

An element is a substance made up of atoms that all have the same number of protons in their nucleus.

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3
Q

To find the number of neutrons in an atom you?

A

Subtract the atomic number from the mass number.

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4
Q

Which number is the mass number and what does it tell you?

A

The top number
It tells you the total number of protons and neutrons in the atom.

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5
Q

Which number is the atomic number and what does it tell you?

A

The bottom number
It tells you the number of protons.

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6
Q

What is an ion?

A

An atom or group of atoms that has lost or gained electrons.

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7
Q

Why do ions have an overall charge?

A

The number of protons do not equal the number of electrons.

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8
Q

Why do atoms not have an overall charge?

A

They have the same number of protons and electrons so the charges cancel out

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9
Q

Number of protons in an atom is equal to?

A

The number of electrons.

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10
Q

The volume of the whats orbit determines the size of the atom?

A

Electrons

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11
Q

Electrons move around the nucleus in?

A

Shells

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12
Q

State the relative mass of protons, neutrons and electrons

A

Protons= 1
Neutrons= 1
Electrons= Almost 0

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13
Q

State the charge of protons, neutrons and electrons

A

Protons= +1
Neutrons= 0
Electrons= -1

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14
Q

Where is most of the mass of the atom concentrated?

A

The nucleus

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15
Q

What is the radius of the nucleus?

A

1x10^-14m

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16
Q

What is the overall charge of the nucleus?

A

Protons + Neutrons = Positive charge

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17
Q

What is the radius of the atom?

A

0.1 nanometres
(1x10^-10m)

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18
Q

Isotopes have the same ________ number but different _______ numbers.

A

Atomic
Mass

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19
Q

How are compounds formed?

A

When elements react atoms combine with other atoms to from compounds.

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20
Q

Define Compound

A

Substances formed by two or more elements, the atoms of each are in fixed proportions throughout the compound and they’re held together by chemical bonds.

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21
Q

What happens when a bond is made?

A

Involves giving atoms away and taking or sharing electrons.

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22
Q

How can you serrate the original elements of a compound?

A

Through a chemical reaction.

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23
Q

What is an ionic compound formed from?

A

One formed from a metal and a non metal.

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24
Q

The metal ion in the compound ______ electrons to form______ ions and the non metal does the opposite.

A

Loses
Positive

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25
Q

What is ionic bonding?

A

The opposite charges of the ions causes a strong attraction.

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26
Q

What does a compound made of non metals consist of?

A

Molecules

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27
Q

What type of bonding is in a molecular compound?

A

Covalent bonding

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28
Q

What is covalent bonding?

A

An atom sharing an electron with another atom

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29
Q

Properties of a compound are different or the same as the original elements

A

Usually completely different

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30
Q

What shows the elements in a compound

A

A formula such as CO2

31
Q

Define nucleus

A

Contains protons and neutrons and nearly the whole mass of the atom is concentrated in the nucleus.

32
Q

What is a mixture?

A

Elements or compounds with no chemical bond between them, that can be separated using physical methods. It does not form new substances.

33
Q

List 5 physical methods of separating mixtures

A

Filtration
Crystallisation
Simple distillation
Fractional distillation
Chromatography

34
Q

How did John Dalton describe atoms?

A

Solid spheres of different elements

35
Q

How did JJ Thompson describe atoms?

A

Plum pudding model
Ball of positive charge with negatively charged electrons embedded in it

36
Q

How did Ernest Rutherford describe atoms?

A

Nuclear model
A tiny positively charged nucleus at the centre where the mass is concentrated. A cloud of negative electrons surround the nucleus. It is mostly empty space.

37
Q

Why was Rutherford wrong?

A

The cloud of negative electrons would be attracted and the atom would collapse.

38
Q

How did Neil’s Bohr describe atoms?

A

Electrons orbit in shells at a fixed distance from the nucleus.

39
Q

Who discovered protons?

A

Rutherford

40
Q

Who discovered neutrons?

A

James Chadwick

41
Q

What was the order of discovery of parts of the atom?

A

Atom
Electrons
Nucleus
Protons
Neutrons

42
Q

What was the order of people atom discovery?

A

Leviticus
John Dalton
JJ Thompson
Ernest Rutherford
Neil’s Bohr
James Chadwick

43
Q

How do you know the electronic structure of an element?

A

Atomic number = protons
Protons = electrons

44
Q

How was the periodic table arranged in early 1800s?

A

Their physical and chemical properties
Their relative atomic mass

45
Q

What is relative atomic mass?

A

The average mass of one atom of an element

46
Q

Who left gaps and predicted elements in the periodic table?

A

Dmitri Mendeleev

47
Q

When did Dmitri make his table?

A

1869

48
Q

How did Mendeleev order his table?

A

Mostly in order of atomic mass but switched order if elements had similar properties.

49
Q

How is the modern periodic table arranged?

A

Increasing atomic (proton) number

50
Q

Which side are metals found?

A

Left

51
Q

What does the group number tell you?

A

The number of electrons in the outer shell

52
Q

Properties of metals

A

Strong
Malleable
Good conductors of heat and electricity
High boiling points and melting points

53
Q

Why are metals more likely to form positive ions when they react?

A

They don’t have many electrons to lose and they need less energy to lose electrons as they have a weaker attraction.

54
Q

Properties of non metals

A

Dull looking and brittle
Some are not solids at room temperature
Don’t conduct electricity They often have a lower density

55
Q

What are transition metals?

A

Typical metals with some additional properties

56
Q

What are the properties of transition metals?

A

Can have more than one ion
Often coloured metal ions
Good catalysts

57
Q

Properties of group 1 elements

A

Very reactive
Soft
Low density
Alkali metals

58
Q

What is the trend of alkali metals as you go down group one?

A

Increasing reactivity
Lower melting point
Lower boiling point
Higher relative atomic mass

59
Q

What do alkali metals and non metals form?

A

Ionic compounds

60
Q

How do group 1 metals react with water?

A

React vigorously to produce hydrogen gas and metal hydroxides, compounds that dissolve in water to produce alkaline solutions

61
Q

How does potassium react with water?

A

Ignites hydrogen

62
Q

How do group 1 metals react with chlorine?

A

React vigorously when heated in chlorine gas to form white metal chloride salts

63
Q

How do group 1 metals react with oxygen?

A

React to form a metal oxide
Lithium forms lithium oxide
Sodium forms a mixture of sodium oxide and peroxide
Potassium reacts to form a mixture of potassium peroxide and superoxide

64
Q

What are the properties of group 7 elements?

A

Halogens
Non metals
Coloured vapours
Molecules or pairs of atoms

65
Q

Properties of fluorine

A

Very reactive
Poisonous
Yellow
Gas

66
Q

Properties of chlorine

A

Fairly reactive
Poisonous
Dense
Green
Gas

67
Q

Properties of bromine

A

Dense
Poisonous
Red brown
Volatile
Liquid

68
Q

Properties of iodine

A

Dark grey
Crystalline
Solid

OR

Purple
Vapour

69
Q

What happens when you go down group 7?

A

The halogens become less reactive
Have higher melting and boiling points
Have higher relative atomic masses

70
Q

What do halogens and non metals form?

A

Molecular compounds
Simple molecular structures

71
Q

What do halogens and metals form?

A

Ionic bonds
Ionic structured compounds

72
Q

When does a displacement reaction occur?

A

Between a more reactive halogen and the salt of a less reactive one

73
Q

Properties of group 0 elements

A

Noble gases
Inert
Colourless at room temperature
Full outer shell
Monatomic gases or single atoms not bonded to each other
Non flammable

74
Q

What happens to group 0 elements as you go down the table?

A

The boiling points increase
The relative atomic masses increase

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