Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

IP Secondary 4 Chemistry > Chapter 1 - The Periodic Table > Flashcards

Chapter 1 - The Periodic Table Flashcards

(114 cards)

Start Studying
1
Q

What is an element?

A

A substance that cannot be split into two or more simpler substances by chemical processes or electricity

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

What does the proton (atomic) number represent?

A

The number of protons in the nucleus of an atom

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

What does the nucleon (mass) number represent?

A

The number of protons and neutrons in the nucleus of an atom

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

How are elements arranged in the Periodic Table?

A

Elements are arranged in order of their increasing proton (atomic) numbers

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

Metals are located on the ________ of the Periodic Table.

A

left and middle

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

Non-metals are located on the ________ of the Periodic Table

inclusive of ________ located at the top of the Periodic Table

A

right

hydrogen

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

Metalloids are located near the ________ between metals and non-metals

A

dividing line

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

What are the metalloids?

A

boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), polonium (Po), astatine (At)

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

How is the group number determined?

A

Determined by the number of valence electrons

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

What do elements in the same group have in common?

A
  • Same number of valence electrons

- Similar chemical properties

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

Elements with 1, 2 or 3 valence electrons (metals) tend to ________ electrons to form ________ charged ions, or ________

A

lose
positively
cations

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

Elements with 5, 6 or 7 valence electrons (non-metals) tend to ________ electrons to form ________ charged ions, or ________

A

gain
negatively
anions

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

How is the period number determined?

A

Determined by the number of electron shells

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

What do elements in the same period have in common?

A

Same number of electron shells

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

Why do the atomic radii of the elements increase down the group gradually?

A

The number of electron shells or energy levels increases down the group as the number of electrons increases.
Each subsequent electron shell or energy level is further away from the nucleus which causes the outer electrons to be more shielded from the attraction of the nucleus (decrease in effective nuclear charge) and less strongly bound, therefore leading to increase of the atomic radii down the group.

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

Why are ionic radii for elements that form positive charge smaller while that for elements that form negative charge larger?

A

As electrons are removed from the outer shell to form positive ion, the attraction for the electrons increases which results in a decrease in ionic radius.
As electrons are added to the outer shell to form negative ion, the repulsion between the electrons causes the ionic radius to increase.

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

Define “metallic character”

A

The tendency of an element to lose electrons and form positive ions (cations)

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

Define “non-metallic character”

A

The tendency of an element to gain electrons and form negative ions (anions)

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

Properties of elements become ________ metallic down the group (i.e. elements lose electrons ________ easily).

A

more

more

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

Properties of elements become ________ metallic from left to right across the period (i.e. elements lose electrons ________ easily).

A

less

less

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

Properties of elements become ________ non-metallic from left to right across the period (i.e. elements gain electrons ________ easily).

A

more

more

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

Group I elements are known as the ________

A

alkali metals

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

What are the Group I metals?

A

lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), francium (Fr)

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

What are the physical properties characteristic of Group I metals?

A
  • Are soft and can be cut by a knife
  • Have a low density (lithium, sodium and potassium float on water)
  • Have relatively low melting and boiling points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What are the physical properties of Group I metals that are typical of most metals?
- Are good conductors of heat and electricity | - Are shiny (seen only when alkali metals are freshly cut)
26
What is the physical properties trend of Group I metals? - Softness ________ down the group - Density ________ down the group - Melting and boiling points ________ down the group
increases increases decrease
27
What are the chemical properties of Group I metals?
Are very reactive
28
What happens in the reaction of alkali metals with oxygen (oxidation)?
Alkali metals react with oxygen in the air to form metal oxides alkali metal + oxygen → alkali metal oxide
29
Oxidation: The rate with which alkali metals react with oxygen in the air ________ down the group - lithium – tarnishes ________ - sodium – tarnishes ________ - potassium – tarnishes ________
increases slowly quickly very quickly
30
Oxidation: How are alkali metals stored?
Stored in oil to prevent them from reacting with oxygen and tarnishing
31
Oxidation: Equation for reaction of lithium with oxygen
lithium + oxygen → lithium oxide | 4Li(s) + O2(g) → 2Li2O(s)
32
Oxidation: Equation for reaction of sodium with oxygen
sodium + oxygen → sodium oxide | 4Na(s) + O2(g) → 2Na2O(s)
33
What happens in the reaction of alkali metals with water?
Alkali metal reacts with water to form a metal hydroxide
34
Reaction with water: Observations for reaction of lithium with water
- Reacts quickly with water - Lithium floats on water - No flame is seen
35
Reaction with water: Equation for reaction of lithium with water
lithium + water → lithium hydroxide + hydrogen | 2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g)
36
Reaction with water: Observations for reaction of sodium with water
- Reacts very quickly with water - Sodium dissolves and darts around the water surface - A yellow flame is seen
37
Reaction with water: Observations for reaction of potassium with water
- Reacts violently with water - Potassium dissolves and darts around the water surface very quickly - A lilac flame is seen
38
Reaction with water: Observations for reaction of rubidium and caesium with water
Violent reactions, which may result in an explosion
39
What is the chemical properties trend of Group I metals? | - Reactivity ________ down the group
increases
40
Compounds of alkali metals: - Have ________ chemical formulae - Have ________ bonds - Are ________ in water
similar ionic soluble
41
Group VII elements are known as the ________
halogens
42
What are the halogens?
fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At)
43
What are the physical properties of halogens?
Have low melting and boiling points | fluorine and chlorine are gases, bromine is a liquid and iodine is a solid at room temperature
44
Why do halogens have low melting and boiling points?
They exist as simple discrete molecules with only weak van der Waals' forces between the molecules
45
What is the physical properties trend of halogens? - Change from a ________ to a ________ down the group - Colour becomes ________ down the group - Melting and boiling points ________ down the group
gas, solid darker increase
46
Why do the melting and boiling points of halogens increase down the group?
The strength of the van der Waals' forces increase due to the increase in relative molecular mass and size of the molecule
47
What are the chemical properties of halogens?
- Are very reactive | - Are diatomic elements
48
Why do halogens exists as diatomic molecules?
- All halogen atoms require one more electron to obtain a full outer shell and become stable - Each atom can achieve this by sharing one electron with another atom to form a single covalent bond
49
What happens in the displacement reactions of halogens?
A halogen takes the place of another halogen in a compound
50
Displacement reaction: What are halides?
Salts in which a halogen reacts with another metal
51
Displacement reaction: A ________ halogen will always displace a ________ reactive halogen from its halides in solution
more | less
52
Displacement reaction: Equation for reaction of fluorine with sodium chloride
fluorine + sodium chloride → sodium fluoride + chlorine | F2(aq) + 2NaCl(aq) → 2NaF(aq) + Cl2(aq)
53
Displacement reaction: Will chlorine and potassium bromide react?
Yes | produces potassium chloride and bromine
54
Displacement reaction: Will chlorine and potassium iodide react?
Yes | produces potassium chloride and iodine
55
Displacement reaction: Will bromine and potassium chloride react?
No
56
Displacement reaction: Will bromine and potassium iodide react?
Yes | produces potassium bromide and iodine
57
Displacement reaction: Will iodine and potassium chloride react?
No
58
Displacement reaction: Will iodine and potassium bromide react?
No
59
What is the chemical properties trend of halogens? | - Reactivity ________ down the group
decreases
60
Halides: - Have ________ chemical formulae - Have ________ bonds - ________ and ________ halides are soluble in water
similar ionic Group I metal, ammonium
61
Group 0 elements are known as the ________
noble gases
62
What are the noble gases?
helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), radon (Rn)
63
What are the physical properties of noble gases?
- Have low melting and boiling points - Are all colourless gases at room temperature - Are insoluble in water
64
What is the physical properties trend of noble gases? | - Melting and boiling points ________ down the group
increase
65
What are the chemical properties of noble gases?
- Have full outer electron shells and do not need to gain, lose or share electrons - Are very stable and chemically unreactive - Are monatomic elements (they exist as individual atoms)
66
Uses of helium
Used in balloons and airships
67
Uses of neon
Used in red glowing advertising signs
68
Uses of argon
Used as a gas blanket in arc wielding Used in fluorescent tubes and low energy light bulbs Used to fill the spaces between the panes in double-glazed windows
69
Uses of krypton
Used in lasers for eye surgery
70
Uses of xenon
Used in sunbeds | Used as a general anaesthetic and in medical imaging as well as in instruments for radiation detection
71
Uses of radon
Used in radiotherapy to treat cancers
72
The block of metals between Groups I and III is known as the ________
transition metals
73
What are the physical properties of transition metals?
- Are lustrous (bright and shiny) - Are hard and strong - Have high densities - Are malleable (can be bent and pressed into different shapes) and ductile (can be drawn into wires) - Are good conductors of heat and electricity - Have high melting and boiling points (except mercury, which is a liquid at room temperature)
74
Compared to the alkali metals, the transition metals are ________ and ________; they ________ be cut with a knife
harder stronger cannot
75
Compared to the alkali metals, the transition metals have ________ density
higher
76
Why are the densities of the transition metals higher than those of the alkali metals?
Transition metals have closed packed structures and relatively small radii. There are more atoms in a fixed volume of transition metal than there are of an alkali metal.
77
Compared to the alkali metals, the transition metals have ________ melting and boiling points, except ________
higher | mercury
78
Why are the melting and boiling points of the transition metals higher than those of the alkali metals?
In alkali metals, only 1 or 2 electrons per atom are delocalised while in transition elements, both 3d and 4s electrons are delocalised as there is a small energy difference between 3d and 4s orbitals. Thus, the metallic bonds are stronger in transition elements.
79
Colour of Cr2+ ion
Sky blue
80
Colour of Cr3+ ion
Green / Violet
81
Colour of Mn2+ ion
Pink
82
Colour of Fe2+ ion
Green
83
Colour of Fe3+ ion
Yellow / Brown
84
Colour of Ni2+ ion
Green
85
Colour of Cu2+ ion
Blue
86
Colour of Cr2O3 oxide
Green
87
Colour of MnO oxide
Black
88
Colour of MnO2 oxide
Black / Brown
89
Colour of FeO oxide
Black
90
Colour of Fe2O3 oxide
Reddish-brown
91
Colour of NiO oxide
Black
92
Colour of CuO oxide
Black
93
Colour of Cu2O oxide
Brick-red
94
Colour of CrO4^2- (chromate)
Yellow
95
Colour of Cr2O7^2- (dichromate)
Orange
96
Colour of MnO4^- (permanganate)
Purple
97
Colour of MnO4^2- (manganate)
Green
98
Colour of MnO3^-
Blue
99
Colour of FeO4^2-
Red
100
Transition metals are ________ reactive than alkali metals
(much) less
101
Transition metals react ________ with air, water and acid
slowly
103
The general trend for transition metals is a ________ in reactivity from left to right across the Periodic Table
decrease
104
Uses of iron
Converted to steel to make cars and buildings
105
Uses of platinum
Used as a catalyst in catalytic converters of cars
106
Uses of copper
Used as roofing material
107
Uses of nickel
Used to make glass frames that can be bent and twisted yet still retaining their shape Used as a catalyst to make margarine
108
Uses of mercury
Used in thermometers and in sphygmomanometer
109
Uses of titanium
Used for hip replacements | Used as a catalyst in making plastics such as cling film
110
Uses of aluminium
Used to make walker (Zimmer frame)
111
Uses of transition metals as catalysts
- Platinum: used in catalytic converters to remove polluting gases (carbon monoxide and nitrogen oxides) from exhausts - Nickel: used as a catalyst in the production of margarine - Iron: used as a catalyst in the production of ammonia from nitrogen and hydrogen via the Haber Process - Titanium: used as a catalyst in the production of plastics
112
Uses of transition metals in building
- Iron: used in building materials due to it being hard, strong, abundant and cheap - Copper: used in electric cables due to good electrical conductivity - Copper: used in plumbing as it is unreactive with water - Copper: a durable roofing material because it reacts slowly with air to form a thin green layer of copper compounds
113
Uses of transition metals in jewellery
- Gold, silver, platinum: used to make jewellery and decoration as they are shiny and do not react with air - Copper: used in bracelets which may ease rheumatic pains
114
Uses of transition metals in medicine
- Titanium: used in artificial joints such as hip replacements (as strong as steel but much lighter and more resistant to corrosion) - Mercury: used in thermometers and also in sphygmomanometer - Platinum: used in platinum-based antineoplastic drugs (chemotherapeutic agents to treat cancer)
115
Uses of alloys (brass and zinc)
- Brass (70% copper and 30% zinc): used to make locks, gears (low friction applications), musical instruments such as horns and bells (high workability and durability) - Steel (iron and other elements such as carbon, nickel and chromium): used to make cutlery, surgical instruments, pressure vessels, handrails etc (due to its high tensile strength, good corrosion resistance and cheap)

IP Secondary 4 Chemistry (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions