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chemistry > Atomic structure and periodic table > Flashcards

Atomic structure and periodic table Flashcards

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1
Q

What is an atom?

A

The smallest part of an element that makes up all matter

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2
Q

What charges do protons, neutrons and electrons have?

A

protons= +1
electrons= -1
neutrons= 0

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3
Q

What is another name for the shell?

A

energy levels

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4
Q

What is an element?

A

a substance made of only atoms with the same number of protons

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5
Q

What is a diatomic molecule/ element?

A

An element where atoms form molecules of 2 of the same atom bonded together

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6
Q

Name some examples of diatomic elements

A

Iodine
Bromine
Chlorine
Fluorine
Oxygen
Nitrogen
Hydrogen

I Bring Clay For Our New House

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7
Q

Wil changing an atom’s number of proton change the atom?

A

Yes, protons give atoms it’s identity

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8
Q

What is a compound?

A

A substance made of at least 2 different elements chemically bonded together

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9
Q

What does the atomic number represent?

A

Protons (same as electrons)

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10
Q

How do you find out number of neutrons?

A

Mass number- atomic number

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11
Q

What is the definition of an isotope?

A

Atoms of the same element with the same number of protons but different numbers of neutrons

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12
Q

What is relative atomic mass?

A

Average mass of an atom taking into account the different masses of the isotopes

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13
Q

How do you work out relative atomic mass?

A

sum of (isotope abundance x isotope mass number) / sum of abundance

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14
Q

What did Democritus discover about matter?

A

All matter were made of small lumps called atoms

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15
Q

What did Dalton discover about the atom?

A

all matter was comprised of
atoms with distinct masses and properties

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16
Q

What did Thomson discover about the atom

A

Discovered electrons. Created plum pudding model. Electrons could be removed.

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17
Q

What was Rutherford’s experiment and what did it prove?

A

Alpha particles scattering experiment
Fired alpha particles at a sheet of gold foil
Proved:
1) atoms are made of mainly empty space
2) the nucleus has a positive charge
3) nucleus is concentrated at the centre
and around this are the electrons

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18
Q

How did Dmitri Mendeleev improv ethe periodic table?

A

Left gaps for undiscovered elements.
Mostly put elements in order of relative atomic mass but switched some around.
These allowed for elements with similar properties to line up in columns.

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19
Q

Do metals form positive or negative ions? What about non-metals?

A

metals= positive
non-metals= negative

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20
Q

How was the periodic table arranged before Mendeleev?

A

In order of relative atomic mass and physical and chemical properties

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21
Q

What does the group number show?

A

number of electrons in outer shell

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22
Q

What does the period number show?

A

number of energy levels (shells)

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23
Q

Describe trends in melting and boiling points of group 1?

A

As you go down group one, melting and boiling point decreases

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24
Q

Describe trends in reactivity of group 1?

A

As you go down group 1, reactivity increases

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25
Q

What does an alkali+ water produce?

A

metal hydroxide+ hydrogen

26
Q

Describe trends in melting and boiling point of group 7?

A

As you go down group one, melting and boiling point increases

27
Q

Describe trends in reactivity of group 7?

A

As you go down group 7, reactivity decreases

28
Q

Describe trends in relative atomic mass of group 7?

A

As you go down group 7, RAM increases

29
Q

Describe trends in relative atomic mass of group 1?

A

As you go down group 1, RAM increases except Ka

30
Q

Describe trends in boiling point of group 0?

A

As you go down group 0, boiling point increases

31
Q

How reactive are noble gasses?

A

Inert/ unreactive because they have a full outer shell

32
Q

What are ions?

A

A charged atom or [article, formed through the loss or gain of an electron

33
Q

How do transition metal gemstones have different colours?

A

They are able to form ions with different charges

34
Q

What is a catalyst?

A

Speeds up a reactions without being used up

35
Q

What is a cation and anion?

A

cation= positive ion
anion= negative ion

36
Q

What is ionic bonding?

A

The electrostatic force of attraction between positively and negatively charged electrons

37
Q

What is ionic bonding between?

A

metal and non- metal

38
Q

What charge ions do group 1, group 2, group 7 form?

A

group 1= +1
group 2= +2
group 7= -1

39
Q

How are ions in ionic compounds arranged?

A

In a lattice

40
Q

Around how many elements are there?

A

100
(118)

41
Q

What is a mixture?

A

Consists of two or more elements or compounds not
chemically combined together. The chemical properties of each
substance in the mixture are unchanged.

42
Q

Which ways can mixtures be separated?
What type of process are these?

A

.Filtration
.Simple distillation
.Evaporation and crystallisation
.Fractional distillation
.Chromatorgrpahy

Physical processes

43
Q

Explain the method of filtration

A

1)Put filter paper into a filter funnel
2)Pour mixture containing insoluble solid
3= liquid passes through into conical flask but solid won’t

44
Q

When would you use filtration?

A

When you want to sperate an insoluble solid from a liquid

45
Q

When would you use simple distillation? Give an example including how it would work

A

When you want to separate a liquid from a solution.
e.g. water from salty water because the water evaporates from the solution
. The salt does not evaporate and so it stays behind

46
Q

Explain the method of simple distillation for water from salty water

A
  1. Salty water is heated
  2. The water vapour cools in the condenser and drips into a beaker
  3. The water has condensed and is now in the beaker, the salt stays behind
47
Q

What did James Chadwick discover?

A

Found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutron

48
Q

Explain the method of evaporation and crystallisation

A

1) slowly heat solution to evaporate to a smaller volume
2)solution will be more concentrated and will be left be left to cool
3)as solution cools, crystals form and can be obtained by filtration

49
Q

When do you use fractional distillation?

A

to separate different liquids from a mixture of liquids

50
Q

Explain the method of fractional distillation

A

1)place mixture in a flask
2) different liquids have different boiling points so you heat the mixture
3)the liquid with the lowest boiling point will evaporate first then you condense it to get the first liquid

51
Q

Explain the method of paper chromatography

A
  1. Ink or plant dye is dotted along the pencil line.
  2. As the paper is lowered into the solvent, some of the dye spreads up the paper

Different substances have different solubilities so will travel at different rates, causing the substances to spread apart

  1. The paper has absorbed the solvent, and the dye has spread further up the paper
52
Q

Explain the two phases of chromatography

A

1)The stationary phase which in paper chromatography is very uniform, absorbent paper
the
2)mobile phase
is the solvent
that moves through the paper, carrying different substances with it

53
Q

What did Bohr discover?

A

Electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus

54
Q

Where is most of the mass in an atom?

A

nucleus

55
Q

Is the mass or atomic number on top?

A

mass

56
Q

How big is the radius of an atom?

A

0.1 x10nm (x10^-10m)

57
Q

How big is the radius of the nucleus?

A

0.1 x 10^-14m

58
Q

True or false:
All elements in group 0 have 8 electrons in their outer shell

A

False
Most do but not all

59
Q

Why do alkali metals get more reactive as you go down?

A

As you go down period 1, the shells increase so the outer shell electrons are further away from the positive charge it is attracted to in the nucleus. Therefore, it is held on more weakly and can be transferred easier.

60
Q

What observations will you see when alkalis react with water?

A

bubbling, flames

61
Q
A

chemistry (3 decks)

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