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Chemistry 21st century > Chemical patterns > Flashcards

Chemical patterns Flashcards

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1
Q

What is constant about all the atoms of a specific element?

A

The number of protons (and therefore electrons unless ionised)

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2
Q

Who thought up the periodic table?

A

Mendeleev.

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3
Q

How is the periodic table organised?

A

Groups (vertical columns) and periods (horizontal rows)

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4
Q

Horizontal means?

A

This way ———————–

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5
Q

Vertical means?

A

Like a tree or a lamp post

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6
Q

How are the elements sorted in the periodic table?

A

Mendeleev used relative atomic masses, we use the proton number

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7
Q

All the elements in a group are?

A

Similar in their chemical reactions.

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8
Q

As you go down the periodic table the nuclei of the elements become?

A

Bigger and heavier

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9
Q

What did the fact not all elements had been discovered mean for Mendeleev’s periodic table?

A

There were gaps

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10
Q

Why were Dobreiner’s triads and Newlands’ octaves rejected?

A

Most elements did not fit their pattern.

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11
Q

How can data about physical properties in the periodic table be used?

A

To make predictions.

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12
Q

When elements are heated they produce…… flames?

A

coloured

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13
Q

What can the coloured light produced by heating an element be split into?

A

A spectrum that is unique to each element.

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14
Q

Name an element that was discovered using spectroscopy?

A

Helium, found on the sun before it was found on earth.

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15
Q

What is in the middle of an atom?

A

A small nucleus.

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16
Q

Where are the electrons in the atom?

A

Travelling around the outside in shells.

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17
Q

What is the charge on a proton?

A

+1

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18
Q

What is the mass of a proton?

A

1

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19
Q

What is the charge on a neutron?

A

0

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20
Q

What is the mass of a neutron?

A

1

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21
Q

What is the charge of an electron?

A

-1

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22
Q

What is the mass of an electron?

A

almost zero

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23
Q

Atoms must have the same number of?

A

Protons and electrons

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24
Q

How do you find the relative atomic mass?

A

Number of protons + number of electrons = relative atomic mass

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25
Q

How are electrons arranged in an atom?

A

In shells around the nucleus.

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26
Q

The shells have space for how many electrons (going out from the nucleus)?

A

2.8.8.18

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27
Q

What is the difference between electrons in different shells?

A

They have different energy levels.

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28
Q

Where would you find the electrons with the lowest energy?

A

Next to the nucleus

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29
Q

What do the elements in group 0 have that makes them inert?

A

Full electron shells.

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30
Q

What happens to the properties of the elements across a period? (Horizontal line)

A

There will be trends.

31
Q

How many electrons are there in the outer shell of the metals?

A

Up to, and including, 3. Note - Hydrogen and Helium are not metals.

32
Q

How many electrons are there in the outer shell of the non-metals?

A

5 or more.

33
Q

If an element has the electron arrangement 2.8.1, what sort of element is it likely to be?

A

A metal

34
Q

What is group 1 called?

A

The alkali metals.

35
Q

What are group 1 metals like?

A

Soft, can be cut with a knife, shiny when first cut, tarnish quickly because they react with oxygen.

36
Q

What happens to properties such as boiling point, melting point, density as you go down the group?

A

They show trends.

37
Q

Metals form bonds by losing their outer electron. Which elements find it easier to lose electrons?

A

The ones where the nucleus is a long way from the electron, so the ones lower in the group.

38
Q

What happens to the reactivity of alkali metals as you go down the periodic table?

A

It goes up.

39
Q

What do group one metals do with water?

A

React - sodium fizzes and moves around, rubidium explodes. Hydrogen is produced.

40
Q

How can you test for hydrogen?

A

It pops when lit.

41
Q

What is left in solution when an alkali metal reacts with water?

A

Alkali metal hydroxide.

42
Q

What colour would you expect an alkali metal hydroxide to turn an indicator?

A

Blue

43
Q

The equation for the reaction of sodium with water is?

A

2Na(s) + 2H2O(l) => H2(g) + 2NaOH(aq)

44
Q

How does sodium react with chlorine?

A

Vigorously, with a bright yellow flame. A white solid is left.

45
Q

What is the white solid produced by the reaction of sodium with chlorine?

A

sodium chloride.

46
Q

Give another name for sodium chloride.

A

Table salt.

47
Q

Which elements are the halogens?

A

Group 7

48
Q

What sort of molecules are the halogen elements?

A

Diatomic

49
Q

The formulae of the halogens are:

A

Cl2; Br2, I2

50
Q

Group 7 elements need to be used in a fume cupboard. Why?

A

They are corrosive and toxic.

51
Q

How do group 7 halogens react with metal?

A

They form halides, eg chloride, bromide, iodide

52
Q

Group 7 halogens need to gain an electron. Which halogens will find this easier?

A

The smaller halogens as the outer shell is closer to the nucleus

53
Q

Where in the periodic table would you find the most reactive halogens?

A

At the top.

54
Q

How many electrons in the outer shell of a halogen?

A

7

55
Q

What is the reaction of metal + halogen?

A

Metal + halogen = > metal halide

56
Q

What happens when a more reactive halogen takes the place of a less reactive halogen?

A

Displacement reaction.

57
Q

Which is more reactive, chlorine or bromine?

A

chlorine

58
Q

Can chlorine displace bromine in a potassium bromide solution?

A

Yes.

59
Q

Can bromine displace chlorine in sodium chloride?

A

No, bromine is less reactive than chlorine and cannot displace it.

60
Q

What are compounds of a group 1 element with a group 7 element like?

A

Solids with high melting points - ionic compounds in a crystal lattice.

61
Q

What do ionic compounds do in water?

A

Dissolve

62
Q

When are the ions free to move in an ionic compound?

A

In solution, or when melted.

63
Q

When can an ionic compound conduct electricity?

A

When dissolved, or melted.

64
Q

How do ionic compounds conduct electricity?

A

The ions move to the electrodes to complete the circuit.

65
Q

How does a group 1 atom become an ion?

A

It loses an electron.

66
Q

How does a group 7 atom become an ion?

A

It gains an electron.

67
Q

Which electron does a group 1 element lose?

A

The one in the outer shell.

68
Q

What charge ions do all group one metals become?

A

+1

69
Q

Where does a halogen ion put the extra electron?

A

Into the outer shell.

70
Q

What is the charge on a halogen ion?

A

-1

71
Q

What is the charge on the OH ion?

A

-1

72
Q

What is the charge on the sulfate (SO4) ion?

A

-2

73
Q

What is the charge on the carbonate (CO3) ion?

A

-2

74
Q

What is the charge on the nitrate ion? (NO3)

A

-1

Chemistry 21st century (10 decks)

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