Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Atomic structure and the periodic table 2 > Flashcards

Atomic structure and the periodic table 2 Flashcards

The periodic table

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards AP® Chemistry flashcards Periodic Table flashcards Organic Chemistry 101 flashcards
1
Q

How were elements classified in the early 1800s?

A

By atomic weight.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What had not been discovered in the early 1800s?

A

Protons
Neutrons
Electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Describe two changes that Mendeleev made to early periodic tables.

A

He left gaps in order to keep elements with similar properties in the same group.

He switched the order of elements based on their properties, even if their atomic weights were no longer in order.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the problems with the early periodic tables?

A

They were incomplete.

Some elements were placed in inappropriate groups if the strict order of atomic weights was followed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What did some of the gaps left by Mendeleev indicate?

A

The existence of undiscovered elements.

Mendeleev could predict what their properties might be.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Elements with properties predicted by Mendeleev were…

A

…discovered and filled the gaps.

When they fit the patterns, this helped confirm Mendeleev’s ideas.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Knowledge of isotopes made it possible to do what?

A

Explain why the order of elements in early periodic tables, based on atomic weights, was not always correct.

Isotopes of the same element have different masses but the same chemical properties so occupy the same position in the periodic table.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What do we call atomic weight now?

A

Relative atomic mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Where does the periodic table get its name?

A

Because similar properties of elements occur at regular intervals - ‘periodically’. This was noticed at early stages.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Date of Dmitri Mendeleev’s table of elements.

A

1869

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How many elements were in Mendeleev’s original table of elements?

A

50

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Give an example of Mendeleev changing the periodic table from order of atomic weight because of the properties of elements.

A

Te and I

Iodine has a smaller atomic weight (relative atomic mass) but is placed after tellurium as it has similar properties to the elements in group 7.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How are the elements of the periodic table arranged?

A

In order of increasing atomic (proton) number.

This means that elements with similar properties are in columns - known as groups.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What do elements in the same group in the periodic table have in common?

A

They have the same number of electrons in their outer shell (outer electrons).

This gives them similar chemical properties.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the vertical columns on the periodic table called?

A

Groups

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How do we work out how many electrons are on the outer shell of atoms of an element?

A

The group number tells you this (1,2,3,4,5,6,7,) apart from group 0.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Elements in the same group are likely to react…

A

…in a similar way.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Using the fact that elements in the same group have similar properties, what can we do?

A

Predict the properties of unknown elements.

Make predictions about reactivity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are the rows called on the periodic table?

A

Periods.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What does the period of an element tell you?

A

How many electron shells there are (start at hydrogen as period 1!)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Chlorine reacts in a similar way to bromine. Suggest a reason why.

A

Both chlorine and bromine are in group 7 and so have the same number of electrons in their outer shell.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Metals

A

Elements that react to form positive ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Non-metals

A

Elements that do not form positive ions when they react.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Are most of the elements in the periodic table metals or non-metals?

A

Metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Where are metals found in the periodic table?

A

To the left and towards the bottom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Where are non-metals found in the periodic table?

A

Towards the right and top.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What do atoms generally react to do?

A

Gain a full outer shell and become stable. They do this by losing, sharing, or gaining electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Why are metals to the left of the periodic table more reactive?

A

They don’t have many electrons to lose so not much energy is needed for the elements to react and form positive ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Why are metals towards the bottom of the periodic table more reactive?

A

Their outer electrons are far from the nucleus so the electrostatic forces of attraction are weaker.

So, not much energy is needed for the elements to react and form positive ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Why is forming positive ions difficult for non-metals?

A

They are either to the right of the periodic table where they have lots of electrons that would have to be lost to gain a full outer shell…

Or towards the top where the outer electrons are close to the nucleus so feel a strong attraction.

It would take a lot of energy to lose the electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is more feasible for non metals to do than lose electrons?

A

Either share or gain electrons to gain a full outer shell.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Why are the basic physical properties of all metals similar?

A

All metals have metallic bonding.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Basic physical properties of metals

A

-Strong

-Malleable

-Good conductors of heat and electricity

-High melting and boiling points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Malleable

A

Can be bent or hammered into different shapes.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Why don’t non-metals have the same properties as metals?

A

They don’t have metallic bonding.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Basic physical properties of non-metals

A

-Dull

-Brittle

-Lower density

-Poor conductors of electricity (generally)

-Aren’t always solids at room temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Non-metals form a variety of different structures, so…

A

…have a wide range of chemical properties.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Where are transition metals found in the periodic table?

A

In the centre.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Transition metals are _____ and have the _____________.

A

Typical metals

Properties you would expect of a ‘proper’ metal: dense, strong, and shiny.

40
Q

What are the special properties of transition metals?

A

-They can have more than one ion

-They are often coloured, and so compounds that contain them are colourful

-They often make good catalysts

41
Q

Example of transition metals with more than one ion

A

Copper forms Cu⁺ and Cu²⁺ ions.
Cobalt forms Co²⁺ and Co³⁺ ions.

42
Q

What transition metal compound is yellow?

A

Potassium Chromate (VI)

43
Q

Which transition metal compound is purple?

A

Potassium (VII) magnate

44
Q

What is a nickel-based catalyst used in?

A

The hydrogenation of alkenes.

45
Q

What is an iron catalyst used in?

A

The Haber process.

46
Q

What are the elements in group 0 of the periodic table called?

A

The Noble Gases.

47
Q

What are the noble gases?

A

Inert, colourless gases (at room temperature).

48
Q

Give examples of group 0 elements.

A

Helium
Neon
Argon

49
Q

Why are the noble gases unreactive?

A

Their atoms have stable arrangements of electrons (eight electrons in their outer shell, except for helium, which has only two electrons).

50
Q

The noble gases do not easily form what?

A

Molecules.

51
Q

Trends as you go down group 0

A

The boiling points of the noble gases increase going down the group (with increasing relative atomic mass).

52
Q

Why does the boiling point of the noble gases increase as you go down the group?

A

The number of electrons in each atom increases as you go down the group.

This means that the intermolecular forces between each atom become greater, which take more energy to overcome.

53
Q

How do we predict the boiling point of an element sandwiched between two other elements with known boiling points?

A

You can predict the boiling point will be halfway between the other two boiling points.

So, add them together and divide by 2.

54
Q

Are the noble gases diatomic?

A

No. They exist as monatomic gases.

55
Q

Monatomic (gases)

A

Single atoms not bonded to each other.

56
Q

Why are the noble gasses non-flammable?

A

They are inert (so don’t react with much at all).

This is because they don’t need to lose or gain outer electrons to become stable.

57
Q

What are the elements in group 1 of the periodic table called?

A

The alkali metals

58
Q

Why do the alkali metals have characteristic properties?

A

Because of the single electron in their outer shell.

59
Q

What are the (similar) properties of all alkali metals?

A

-Soft

-Low density

-Low melting and boiling points

60
Q

The alkali metals are…

A

Very reactive!

61
Q

Trends as you go down group 1

A

-Reactivity increases

-Lower melting and boiling points

-Higher relative atomic mass

62
Q

Why does the reactivity of group 1 elements increase as you go down the periodic table?

A

The electron shells become further away from the nucleus.

This means that the electrostatic forces are weaker.

Which means the outer electron is more easily lost.

63
Q

What type of compound do alkali metals form?

A

Ionic compounds with non-metals.

64
Q

What is the charge on the ion of an alkali metal?

A

1+

65
Q

What are ionic compounds?

A

(generally) white solids that dissolve in water to form colourless solutions.

66
Q

How do group 1 (alkali metals) react when placed in water?

A

Vigorously.

As we go down group 1, the reactions become more violent because the metals are more reactive.

67
Q

Alkali metal + Water → What products?

A

Metal hydroxide + Hydrogen

68
Q

Symbol equation for reaction of sodium with water.

A

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

69
Q

What are metal hydroxides?

A

Metal compounds that dissolve in water to produce alkaline solutions.

70
Q

The amount of energy given out by the reaction of an alkali metal with water…

A

…increases down the group.

The reaction with potassium releases enough energy to ignite hydrogen.

71
Q

How do group 1 (alkali metals) react when heated chlorine gas?

A

Vigorously.

72
Q

Alkali metal + Chlorine → What product?

A

Metal chloride salts e.g. sodium chloride.

73
Q

Symbol equation for the reaction of sodium heated in chlorine gas.

A

2Na (s) + Cl₂ (g) → 2NaCl (s)

74
Q

Alkali metal + Oxygen → What product?

A

Metal oxide

(the type will differ depending on the Group 1 metal used).

75
Q

What does Lithium react with oxygen to form?

A

Lithium oxide (Li₂O).

76
Q

What does Sodium react with oxygen to form?

A

A mixture of sodium oxide (Na₂O) and sodium peroxide (Na₂O₂).

77
Q

Sodium peroxide

A

Na₂O₂

78
Q

What does Potassium react with oxygen to form?

A

A mixture of potassium peroxide (K₂O₂) and potassium superoxide (KO₂).

79
Q

potassium peroxide

A

K₂O₂

80
Q

potassium superoxide

A

KO₂

81
Q

Are group 1 metals or transition metals more reactive?

A

Group 1 (alkali) metals.

They react more vigorously with water, oxygen, and group 7 elements, for example.

82
Q

Group 1 vs Transition metals

A

-Group 1 (alkali) metals are less dense, strong, and hard than transition metals.

-Group 1 metals have much lower melting points than transition metals (manganese = 2000°C vs sodium =98°C).

83
Q

What are the elements in group 7 of the periodic table called?

A

The halogens

84
Q

Why do the halogens have similar reactions?

A

Because they all have 7 electrons in their outer shell.

85
Q

Are the halogens diatomic?

A

Yes

85
Q

Diatomic

A

Molecules made of pairs of atoms.

86
Q

What are the 7 diatomic elements?

A

hydrogen, nitrogen, oxygen, fluorine, chlorine, iodine, bromine

87
Q

Trends as you go down group 7

A

As you go down group 7, the halogens:

-become less reactive
-have higher melting and boiling points
-have higher relative atomic masses

88
Q

What are the halogens?

A

Non-metals with coloured vapours.

89
Q

Fluorine (F₂)

A

A very reactive, poisonous yellow gas.

90
Q

Chlorine (Cl₂)

A

A fairly reactive, poisonous dense green gas

91
Q

Bromine (Br₂)

A

A dense, poisonous, red-brown volatile liquid

92
Q

Iodine (I₂)

A

A dark grey crystalline solid or a purple vapour.

93
Q

A more reactive halogen can displace a less reactive halogen from what?

A

An aqueous solution of its salt (a bromide or iodide).

94
Q

What type of compounds do the halogens form?

A

Covalent bonds with other non-metals, forming simple covalent structures.

Ionic bonds with metals, forming ionic structures.

95
Q

What type of ions do halogens form?

A

1- ions called halides (F-, Cl-, Br-, and I-)

96
Q

What do HCl, PCl₅, HF, and CCI₄ have in common?

A

They all contain covalent bonds and contain halides.

Chemistry (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions