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Chemistry > Topic 1 Atoms > Flashcards

Topic 1 Atoms Flashcards

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1
Q

What is an atom

A

Smallest part of an element that can’t be divided

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2
Q

What is an element

A

A substance that contains atoms that all have the same number of protons. Contains one type of atom .

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3
Q

What is a compound

A

Two or more elements held by chemical bonds that take place in a chemical reaction. There is a detectable energy change, and at least one new substance is made. The atoms are held in fixed proportions.

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4
Q

What is a mixture

A

Two or more elements or compounds not in a chemical bind and can be separated by physical methods e.g. SiO2 sand from water using filtration, salt from water using distillation or evaporation. Chemical properties remain the same

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5
Q

What is a molecule

A

Two or more atoms bonded together that can be elemental molecule ( the same type) or a compound molecule ( different types)
E.g. O2 and CO2

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6
Q

What is an isotope

A

Different forms of the same element that have the same number of protons and electrons but a different number of neutrons

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7
Q

What is relative atomic mass

A

Top number

Average of the isotopes of an elements abundances and masses

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8
Q

What is the charge of the nucleus

A

Positive

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9
Q

What is the charge of an atom

A

Neutral because the number of protons equal the number of electrons so the charges cancel out they have the same size charges

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10
Q

What is the radius of an atom

A

1x10-10

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11
Q

Where is the mass concentrated

A

The whole mass is concentrated in the nucleus

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12
Q

How do electrons move

A

Electrons move around in shells round the nucleus

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13
Q

What is the mass and charges of p e and n

A

P. 1. +1
E. 1/2000. -1
N. 1. 0

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14
Q

What are the radicals and valencies

A 
Group no is valency 
Sulphate SO4        2 
Ammonium NH4    1
Hydroxide   OH.     1
Nitrate.        NO3.   1
Carbonate.  CO3.   2
Hydrogen carbonate HCO3 1
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15
Q

Why do we balance equations

A

To end up with the same amount of atoms from start till finish

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16
Q

Describe dobereiners triads

A

Ordered them in atomic mass
Some elements shared similar properties so put them into groups of three called triads
The atomic weight of the middle element was the average of the top and bottom elements
It didn’t work out because New elects were discovered

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17
Q

Describe newlands method

A

Increasing atomic weight
Noticed similar properties amongst every eighth element law of octaves
Patterns were repeated e.g. Reactive metal and was followed eight places later by reactive metal K

18
Q

Why didn’t newlands work out

A

Didn’t leave spaces for undiscovered elements
Ordering in atomic weight some were put in the same group e.g. K in front of Ar
Some occupied the same space

19
Q

What did Mendeleev do different

A

He put them in increasing atomic weight but left gaps
He made sure elements with similar properties were in the same group
Leaving gaps could help him predict undiscovered elements and what their properties might be

20
Q

What discovery showed that Mendeleev was right not to place elements in order of relative atomic mass

A

Isotopes to not put everything in a strict order but to also take into account properties
Isotopes of the same element have different masses but have the same chemical properties so occupy the same position

21
Q

How is the modern periodic table ordered

A

It’s ordered in atomic number

22
Q

Why is it called the periodic table

A

Patterns are repeated in properties

23
Q

Why are elements placed in the same group

A

Because they have similar properties

24
Q

What does the group number mean why is this useful

A

How many electrons there are in the outer shell

As the way atoms react depends on the number of electrons in outer shell

25
Q

What does the period number mean

A

How many electron shells an atoms has

26
Q

If you know the properties of one elements

A

You can predict properties of other elements

27
Q

Properties of transition metals

A 
High density
Conductors of heat and electricity
Have more than one ion- often coloured
Compounds are colourful
Can be used as catalysts 
Can be bent
28
Q

Properties of metals

A 
Shiny 
Malleable 
Ductile 
Sonorous
Conductors of heat and electricity
29
Q

Properties of alkali metals

A

Soft can be cut with knife
Less dense so can float on water
Dull when reacting with oxygen
All have one electron in their outer shells- very reactive have similar properties

30
Q

What happens as you go down group one

A

Reactivity increases
Outer electron more easily lost as the electrostatic attraction between the nucleus and electron decreases because the electron is further away from the nucleus
Melting points decrease going down the group

31
Q

What happens when an alkali metal reacts with water

A

It produces a metal hydroxide and hydrogen gas the salts dissolve to make an alkali solution

32
Q

What happens to an alkali metal when reacting with chlorine

A

It reacts vigorously when heated with chlorine gas to make white metal chloride salts

33
Q

Alkali metal with oxygen

A

Metal oxide

34
Q

Group 7 halogens diatomic molecules

A

F yellow gas
Cl. Green gas
Br brown liquid
I. Purple vapour

35
Q

What do the halogens exist as

A

They all exist as molecules which are pairs of atoms

36
Q

What do halogens have in common

A

All have seven electrons in their outer shell

37
Q

Trends going down the group 7

A

As you go down they become less reactive because the electron cannot be easily gained as it is further away from the nucleus
Higher melting and boiling points

38
Q

What happens when halogens bond with a metal

A

They form a negative halide ion

They take place in displacement reactions

39
Q

What is the goal of atoms

A

The goal of atoms is to have a full outer shell and they do this by reacting

40
Q

Group 0

A

Noble gases

41
Q

Why are group 0 not reactive

A

They are inert because they have a full outer shell

42
Q

Properties of noble gases

A

Monatomic gases
Colourless gases at room temperature
Aren’t flammable because they don’t react
Boiling points increase going down the group

Chemistry (2 decks)

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