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Chemistry Unit 3 IB

Total questions: 99

Worksheet time: 59mins

Name
Class
Date
1.

elements in the periodic table are placed in order of increasing......

a)

mass number

b)

relative atomic mass

c)

atomic mass

d)

relative mass number

2.

why can we assume we've found all the natural elements

a)

there are no gaps in the sequence of the periodic table

b)

everything on the periodic table fits perfectly together

c)

the atomic number increases

d)

because none more can be found

3.

columns are also known as...

a)

periods

b)

groups

4.

rows are also known as...

a)

periods

b)

groups

5.

elements whose valence electrons occupy an s-sublevel are in the...

a)

metals section

b)

first period

c)

first group

d)

s-block

6.

identify the blue block

a)

s-block

b)

p-block

c)

d-block

d)

f-block

7.

identify the yellow block

a)

s-block

b)

p-block

c)

d-block

d)

f-block

8.

identify the red block

a)

s-block

b)

p-block

c)

d-block

d)

f-block

9.

identify the green block

a)

s-block

b)

p-block

c)

d-block

d)

f-block

10.

electron configuration of sodium

a)

3s2

b)

3s1

c)

3p2

d)

4s2

11.

Characteristics of metals

a)

Low conductivity

b)

not ductile + malleable

c)

gas at room temp

d)

good conductors of heat and electric current

e)

brittle + dull

12.

Characteristics of non-metals

a)

Low conductivity

b)

not ductile + malleable

c)

gas at room temp

d)

good conductors of heat and electric current

e)

brittle + dull

13.

metalloids

a)

Elements that have properties of both metals (physically) and nonmetals (chemically).

b)

Elements that have properties of both metals (chemically) and nonmetals (physically).

c)

Elements that have properties of metals

d)

Elements that have properties of nonmetals

14.

lathanoides and actinoides

a)

found in s-block

b)

found in p-block

c)

found in d-block

d)

found in f-block

15.

what are the metalloids

a)

As, Sb, Te

b)

B, Si, Ge, As, Sb, Te

c)

B, Si, Ge,

d)

B, Si, Gn, As, Sb, Ti

16.

Which properties increase in value when descending group 1?

I. First ionization energy

II. Atomic radius

III. Reactivity with water

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

17.

Ionization energy _____ across period

a)

increases

b)

decreases

18.

Electron Affinity _____ across period

a)

increases

b)

decreases

19.

Atomic Radius _____ across period

a)

increases

b)

decreases

20.

Atomic Radius _____ down the group

a)

increases

b)

decreases

21.

Electron Affinity _____ down the group

a)

increases

b)

decreases

22.

Ionization Energy _____ down the group

a)

increases

b)

decreases

23.

non-metallic character _____ diagonally across the group

a)

increases

b)

decreases

24.

metallic character _____ diagonally across the group

a)

increases

b)

decreases

25.

Effective Nuclear Charge _____ across period

a)

increases

b)

decreases

26.

relative charge experienced by outer-electrons is _____ than/to full nuclear charge

a)

less

b)

more

c)

equal

27.

Why is the relative charge experienced by outer-electrons less than full nuclear charge of the atom?

a)

electrons are attracted by inner electrons

b)

electrons are further away from the nucleus

c)

electrons are further away from the protons

d)

electrons are repelled by inner electrons

28.

trends in ionic radius

a)

positive ions smaller than parent ions, formation of positive ions involves loss of outer shell

b)

negative ions are larger than parent ions, addition of electrons into shell increased repulsion between electrons in outer principle energy causing electrons to move further apart

c)

ionic radii decreases from groups 1-14 for positive ions due to increase in nuclear charge across the period, increased attraction between nucleus + electrons pulls outer shell closer to nucleus

d)

ionic radii decreases for negative ions groups 14-17, due to increase in nuclear charge across period, positive ions are smaller than negative ions

e)

ionic radii increase down a group as number of electron energy levels increase

29.

ionization energy trends

a)

ionization energies decrease down a group, the electron is removed from the energy level furthest from the nucleus, nuclear charges increase but the effective nuclear charge is the same due to shielding of inner electrons so distance increases between electron + nucleus reducing attraction between them

b)

decreases for negative ions groups 14-17, due to increase in nuclear charge across period, positive ions are smaller than negative ions

c)

negative ions are larger than parent ions

d)

ionization energy increases across a period, an increase in effective nuclear charge causes an increase in attraction between outer electrons and nucleus and makes it electrons difficult to move

30.

Why are Electron Affinity values not available for noble gases?

a)

as they don’t generally form negatively charged ions

b)

As noble gases are unreactive

c)

as they don't have the ability to form bonds with other atoms

d)

as they are neglible

31.

electronegativity

a)

a measure of ability of atom to repel electrons in a covalent bond

b)

a measure of ability of atom to attract electrons in a covalent bond

c)

measure of repulsion between nucleus + outer-electrons (bonding electrons)

d)

measure of attraction between nucleus + outer-electrons (bonding electrons)

e)

a measure of ability of atom to attract electrons in an ionic bond

32.

an element with high electronegativity has - electron pulling power

a)

weak

b)

strong

33.

why does electronegativity increase across the period

a)

due to an increase in nuclear charge resulting in increased attraction between the nucleus and bond electrons

b)

due to a decrease in nuclear charge resulting in increased attraction between the nucleus and bond electrons

c)

due to an increase in nuclear charge resulting in a decreased attraction between the nucleus and bond electrons

d)

due to an increase in nuclear charge resulting in increased attraction between the nucleus and bonding electrons of other elements

34.

highest value of electronegativity

a)

manganese

b)

caesium

c)

flourine

d)

francium

35.

lowest value of electronegativity

a)

manganese

b)

caesium

c)

flourine

d)

francium

36.

Properties of Ionization Energies

a)

measured directly

b)

properties of atoms in a molecules

c)

derived indirectly from experimental bond energy data

d)

property of gaseous atoms

e)

elements with high ionization energy have the most exothermic electron affinities

37.

Properties of Electronegativity

a)

measured directly

b)

properties of atoms in a molecules

c)

derived indirectly from experimental bond energy data

d)

property of gaseous atoms

e)

elements with high electronegativity have the most exothermic electron affinities

38.

Melting points of different elements depend on their...

a)

bonding

b)

electron affinity

c)

structure

d)

electronegativity

e)

ionization energy

39.

Chemical Properties are determined by the elements...

a)

effective nucleir charge

b)

ionization energy

c)

melting point

d)

electron configuration

40.

Characteristics of Noble Gases

a)

they’re colourless gases

b)

diatomic; exist as two atoms

c)

monatomic; exist as single atoms

d)

very unreactive

e)

in group 18

41.

the lack of reactivity of noble gases is due to...

a)

them not usually forming negative ions as they have the highest ionization energy

b)

them not usually forming positive ions as they have the highest ionization energy

c)

easily gain/lose electrons thus making the energy release neglible

d)

them not forming negative ions as extra electrons have to be added to the outer energy level shell where they’d experience neglible effective nuclear force with protons shielded by the equal number of inner electrons

42.

with exception of _____ noble gases all have complete valence energy levels with eight electrons

a)

neon

b)

helium

c)

argon

d)

xenon

43.

noble gases all have complete valence energy levels with ____ electrons

a)

4

b)

7

c)

8

d)

10

44.

The term “ (a)   ” describes the fact that many atoms in molecules are most stable when the valence shell contains effectively eight electrons

45.

reactivity ____ down group

a)

increases

b)

decreases

46.

the reactivity of elements in other groups can be explained by.....

a)

stable complete electron energy levels

b)

unstable complete electron energy levels

c)

stable incomplete electron energy levels

d)

unstable incomplete electron energy levels

47.

Why are alkali metals stored in oil?

a)

to ensure the preservation of their properties

b)

to prevent contact with air and water

c)

to maintain the metals properties

d)

metals thrive in oil based substances

48.

Physical Properties of Alkali Metals

a)

good conductors of electricity + heat

b)

low densities

c)

high densities

d)

grey shiny surfaces when freshly cut with a knife

e)

very reactive metals

49.

Chemical Properties of Alkali Metals

a)

good conductors of electricity + heat

b)

unreactive metals

c)

similar chemical properties to noble gases

d)

form ionic compounds with non-metals

e)

very reactive metals

50.

Why are alkali metals able to conduct heat and electricity

a)

due to the mobility of their inner electrons

b)

due to their high densities

c)

due to their low densities

d)

due to the mobility of their outer electron

51.

Alkali metals react with water to produce:

a)

nitrogen

b)

hydrogen

c)

carbonate

d)

metal nitrate

e)

metal hydroxide

52.

What happens when you drop lithium in water?

a)

floats

b)

sinks

c)

reacts slowly

d)

releases hydrogen

e)

keeps its shape

53.

What happens when you drop sodium in water?

a)

the heat produced is sufficient enough to ignite the hydrogen produced, which produces a lilac coloured flame and moves excitedly on surface

b)

the heat produced is sufficient enough to melt the unreacted metal which forms small ball and moves around on the water's surface

c)

reacts slowly

d)

reacts vigorously

e)

releases hydrogen

54.

What happens when you drop potassium in water?

a)

the heat produced is sufficient enough to ignite the hydrogen produced, which produces a lilac coloured flame and moves excitedly on surface

b)

the heat produced is sufficient enough to melt the unreacted metal which forms small ball and moves around on the water's surface

c)

reacts slowly

d)

reacts very vigorously

e)

releases hydrogen

55.

halogens exist as...

a)

monoatomic molecules

b)

diatomic molecules

c)

triatomic molecules

56.

Physical Properties of Halogens

a)

coloured

b)

colourless

c)

high densities

d)

show gradual change from gases to solids

e)

very reactive metals

57.

Chemical Properties of Halogens

a)

reactivity decreases down the group

b)

reactivity increases down the group

c)

form ionic compounds with metals and covalent compounds with other non-metals

d)

form ionic compounds with non-metals and covalent compounds with metals

e)

very reactive non-metals

58.

halogens + group 1 → _______

a)

hydrogen

b)

ionic compounds

c)

ionic halides

d)

hydroxide

59.

most vigorous attraction occurs between elements which are the _________ on periodic table

a)

furthest apart

b)

closest to each other

60.

halogens form _____ salts w silver

a)

soluble, causing a reaction which produces a hydrogen and hydroxide

b)

soluble, causing a colour changing reaction that's useful in identifying the halide ion

c)

insoluble, causing a build-up of solute at the bottom of the solution

d)

insoluble, causing a precipitate that’s useful in identifying halide ion

61.

smaller atomic radius means that...

a)

the nucleus has a stronger attraction for electrons

b)

the nucleus has a weaker attraction for electrons

62.

_____ compounds are generally formed between metals and non-metals so oxides of elements Na-Al have _______

a)

ionic, molecular ionic structures

b)

covalent, giant covalent structures

c)

covalent, molecular covalent structure

d)

ionic, giant ionic structures

63.

______ compounds formed between non-metals so oxides of phosphurus+sulfur+chlorine are ________

a)

ionic, molecular ionic structures

b)

covalent, giant covalent structures

c)

covalent, molecular covalent structure

d)

ionic, giant ionic structures

64.

oxide of silicone (metalloid) gas has a _________

a)

ionic, molecular ionic structures

b)

covalent, giant covalent structures

c)

covalent, molecular covalent structure

d)

ionic, giant ionic structures

65.

metallic elements which form ionic oxides are ______

a)

basic

b)

acidic

c)

amphoteric

66.

non-metal oxides that are covalent are ______

a)

basic

b)

acidic

c)

amphoteric

67.

aluminium oxide is ______

a)

basic

b)

acidic

c)

amphoteric

68.

Basic Oxides reacts with ________

a)

water to produce acidic solutions

b)

an acid to form a salt and water

c)

acts as a base when reacting with acid, acts as an acid when reacts with alkalis

69.

Acidic Oxides/non-metallic oxides react with ________

a)

water to produce acidic solutions

b)

an acid to form a salt and water

c)

acts as a base when reacting with acid, acts as an acid when reacts with alkalis

70.

Amphoteric Oxides ________

a)

reacts with water to produce acidic solutions

b)

reacts with an acid to form a salt and water

c)

acts as a base when reacting with acid, acts as an acid when reacts with alkalis

71.

Metals Have ______ Ionization Energies and Electronegativities than Non-Metals

a)

lower

b)

higher

72.

Chemical Properties of Transition Metals

a)

→ they form compounds with a variable oxidation state

→ they form a variety of complex ions

→ they form coloured compound

→ they act as catalysts when either elements or compounds

→ they have magnetic properties

b)

→ they form compounds with a variable oxidation state

→ they form a few complex ions

→ they form colourless compounds

→ they act as catalysts when either elements or compounds

→ they have magnetic properties

c)

→ they form compounds with a variable oxidation state

→ they form a few complex ions

→ they form coloured compounds

→ they act as catalysts with elements and not compounds

→ they don't have magnetic properties

d)

→ they form compounds with a variable oxidation state

→ they form coloured compounds

→ they act as catalysts with elements and not compounds

→ they don't have magnetic properties

73.

Which of the following is not a transition metal?

a)

copper

b)

chromium

c)

vanadium

d)

zinc

74.

why is zinc NOT considered to be a transition metal?

a)

it is magnetic

b)

only forms white compounds

c)

it does have a partially filled d sub-level

d)

Zinc only forms one ion

e)

it does not have a partially filled d sub-level

75.

a substance which alters the rate of reaction by providing an alternative reaction pathway with a lower activation energy

(a)  

76.

Which of the following is used in catalytic converters?

a)

manganese hydroxide

b)

platinum

c)

phosphorus

d)

palladium

e)

gold

77.

ferromagnetism

a)

The property that allows a substance to become permanently magnetized when placed in a magnetic field; exhibited by iron, cobalt, and nickel and some of their alloys.

b)

a type of induced magnetism, associated with unpaired electrons, that causes a substance to be attracted into the inducing magnetic field

c)

a type of magnetism, associated with paired electrons, that causes a substance to be repelled from the inducing magnetic field

78.

paramagnetism

a)

The property that allows a substance to become permanently magnetized when placed in a magnetic field; exhibited by iron, cobalt, and nickel and some of their alloys.

b)

a type of induced magnetism, associated with unpaired electrons, that causes a substance to be attracted into the inducing magnetic field

c)

a type of magnetism, associated with paired electrons, that causes a substance to be repelled from the inducing magnetic field

79.

diamagnetism

a)

The property that allows a substance to become permanently magnetized when placed in a magnetic field; exhibited by iron, cobalt, and nickel and some of their alloys.

b)

a type of induced magnetism, associated with unpaired electrons, that causes a substance to be attracted into the inducing magnetic field

c)

a type of magnetism, associated with paired electrons, that causes a substance to be repelled from the inducing magnetic field

80.

the type of magnetism of Iron (II) complex ion when containing a weak ligand

a)

ferromagnetism

b)

paramagnetism

c)

diamagnetism

81.

the type of magnetism of Iron (II) complex ion when containing a strong ligand

a)

ferromagnetism

b)

paramagnetism

c)

diamagnetism

82.

neutral ions or anions containing a non-bonding pair of electrons which can form co-ordinate covalent bonds with a metal ion to form a complex ion

(a)  

83.

ligands ____ be replaced by other ligands

a)

can

b)

cannot

84.

the number of lone pairs bonded to the metal ion

(a)  

85.

compounds with coordination number of 6 have a ______ shape

a)

linear

b)

tetrahedal

c)

octahedral

d)

square planar

86.

compounds with coordination number of 2 have a ______ shape

a)

linear

b)

tetrahedal

c)

octahedral

d)

square planar

87.

factors affecting colour of transition metal complexes

a)

identity of ligand

b)

oxidation state

c)

the electron configuration of the element

d)

nature of transition element

e)

stereochemistry of the complex

88.

what you can find out about the complex using its colour

a)

charge of metal ion

b)

identity of ligand

c)

oxidation state of metal ion

d)

coordinate number

e)

identity of metal ion

89.

Why do transition metal complex ions show a colour

a)

the metal ions have a corresponding colour corresponding to their strength

b)

the ligands have a corresponding colour corresponding to their strength

c)

because the splitting of the d-levels caused by the ligand corresponds to a certain wavelength therefore omitting a visible colour

d)

because the splitting of the s-levels caused by the ligand corresponds to a certain wavelength therefore omitting a visible colour

90.

big delta E means

a)

big jump

b)

small jump

c)

big energy absorbed (higher colour)

d)

small energy absorbed (lower colour)

91.

small delta E means

a)

big jump

b)

small jump

c)

big energy absorbed (higher colour)

d)

small energy absorbed (lower colour)

92.

more protons results in a _____ split

a)

bigger

b)

smaller

93.

the smaller the oxidation state the _____ the split

a)

smaller, (absorbs lower energy)

b)

bigger, (absorbs higher energy)

94.

high energy =

a)

high frequency

b)

low frequency

95.

if red/orange light is absorbed the solution appears

a)

red-orange

b)

blue-green

c)

red-yellow

d)

blue-purple

96.

which one is correct (lowest to highest energy)

a)

Red →Orange → Yellow → Green→ Light Blue → Blue → Violet

b)

Red →Yellow→ Orange → Green→ Blue → Light Blue → Violet

c)

Red →Orange → Yellow → Green→ Blue → Light Blue → Violet

d)

Violet →Orange → Yellow → Green→ Light Blue → Blue → Red

97.

Weak ligands

a)

NCS- to CO

b)

I- to H2O

98.

Strong ligands

a)

NCS- to CO

b)

I- to H2O

99.

Strong ligands

a)

NCS- to CO

b)

I- to H2O

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