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Quiz Sr3ScA & C (2023)

Total questions: 100

Worksheet time: 2hrs 52mins

Name
Class
Date
1.

An equal volume of two gases is mixed together and a vigorous reaction occurs at room temperature and pressure conditions. What are the two gases?

a)

Nitrogen and hydrogen

b)

Hydrogen and oxygen

c)

Hydrogen and fluorine

d)

Chlorine and hydrogen

2.

Which of the following ions will show a lilac colour flame when heated.

a)

Ca2+

b)

Cu2+

c)

Na+

d)

K+

3.

Which of the following statements about the compound of Group 2 elements from magnesium to barium is correct?

a)

Carbonates of Group 2 elements produce bubbles when added to dilute nitric acid

b)

Nitrates of Group 2 elements produce nitrogen gas and oxygen gas on heating

c)

Oxides of Group 2 elements produce bubbles when added to dilute hydrochloric acid

d)

The oxides of group 2 elements are amphoteric

4.

A 5.00 g sample of an anhydrous Group 2 metal nitrate loses 3.64 g in mass when heated strongly. Which metal is present?

a)

Magnesium

b)

Calcium

c)

Strontium

d)

Barium

5.

Which of the following compounds show amphoteric properties?

a)

Ca(OH)2

b)

NaOH

c)

Mg(OH)2

d)

Al2O3

6.

Electron configuration of X is: 1s2 2s2 2p6 3s2 3p4. What is the formula of compound formed when sodium reacts with X?

a)

NaX

b)

NaX2

c)

Na2X

d)

Na2X3

7.

Which of the followings particles difficult to remove its valence electrons?

a)

Ar(g)

b)

Cl-(g)

c)

Ca+(g)

d)

Na+(g)

8.

In the Periodic table of elements, the most reactive metal atom comprises of

a)

Large atomic radius and low electronegativity

b)

Large atomic radius and high electronegativity

c)

Small atomic radius and low electronegativity

d)

Small atomic radius and high electronegativity

9.

Which of the following reactions showed the reaction happened when the lime mortar used to paint the walls is solidify.

a)

CaO(s) + H2O(l) --> Ca(OH)2(s)

b)

CaCO3(s) --> CaO(s) + CO2(g)

c)

Ca(OH)2(s) + CO2(g) --> CaCO3(s) + H2O(l)

d)

Ca(HCO3)2(s) --> CaCO3(s) + H2O(l) + CO2(g)

10.

If a metal soluble in dilute H2SO4 to give H2, but it hydroxide compound unable to soluble in excess NaOH. The metal is?

a)

Zn

b)

Mg

c)

Be

d)

Cr

11.

Which statement correctly describes the trend in properties on descending Group 2 (from Mg to Ba)?

a)

The solubility in water decrease down the group 2

b)

The first ionisation energy increases

c)

The ionic radius decreases

d)

The solubility of sulphate increases

12.

Which set of solid elements includes giant metallic structure, macromolecular structure and simple molecular structure?

a)

Na, Mg, Al

b)

Mg, Al, Si

c)

Al, Si, S

d)

Si, P, S

13.

Which of the following statements correctly described the properties of group 1 elements?

a)

I, II and III

b)

I, II and IV

c)

II, III and IV

d)

III and IV

14.

Which of the following diagrams correctly shows the electronegativity of the elements Na, Mg, Al and Si plotted against their first ionization energies?

a)

b)

c)

d)

15.

The graph shows the part of the successive ionisation energies of element X and element Y. Both elements are in Period 3.

a)

An atom of element X needs one extra electron for a full outermost shell; an atom of element Y needs two extra electrons for a full outermost shell

b)

Element X has an oxidation number of +7 in most of its compounds

c)

An atom of element Y has five electrons in the 3rd shell

d)

When element X combines with element Y, the bonding is ionic.

16.
An example of elements from period 3 that have the same number of electron shell
a)
Hydrogen and Oxygen
b)
Sodium and Potassium
c)
 Sodium and Magnesium
d)
Helium and Hydrogen
17.
 Groups contain the same amount of ___________________ electrons, and periods contain the same number of ____________________shell.
a)
 atom/ electron
b)
valence/electron
c)
electron /valence
d)
protons/neutrons  
18.

______________________is formed when metal reacts with water.

a)

non-metal hydroxide

b)

metal hydroxide

c)

hydride

d)

metal oxide

19.

Impure Hydrogen burns with

a)

pop sound

b)

blue flame

c)

pop sound as it contains impurities.

d)

silent

20.

Addition of hydrogen to vegetable oil to get vanaspati ghee in presence of catalyst.

a)

hydrogenation

b)

catalytic hydrogenation

c)

catalysis

d)

catalytic dehydration

21.

What is False about ice-

a)

Its density is more than water

b)

A water molecule form 4 H-Bond

c)

It is a thermal insulator

d)

Its density is less than water

22.

Hydrogen can be obtained from water, by the action of water on-

a)

Calcium carbide

b)

Calcium hydride

c)

Calcium oxide

d)

Calcium chloride

23.

Metal hydrides are ionic, covalent or molecular in nature. Among LiH, NaH, KH, RbH, CsH, the correct order of increasing ionic character is

a)

LiH > NaH > CsH > KH>RbH

b)

LiH < NaH < KH < RbH < CsH

c)

RbH > CsH > NaH > KH > LiH

d)

NaH > CsH > RbH > LiH > KH

24.

Dihydrogen can be prepared on commercial scale by different methods. In its preparation by the action of steam on hydrocarbons, a mixture of CO and H gas is formed. It is known as________________

a)

CO2 + H2

b)

Syngas

c)

Producer gas

d)

Industrial gas

25.

Select two correct answers. Going the down Group 1,

a)

Reactivity increases

b)

Atomic size decreases

c)

Electropositivity increases

d)

Density decreases

26.

Explain why reactivity increases going down Group 1.

a)

Atomic size increased, and the force of attraction between nucleus and valence electron increased.

b)

Atomic size decreased, and the force of attraction between nucleus and valence electron decreased.

c)

Atomic size increased, and the force of attraction between nucleus and valence electron decreased.

d)

Atomic size decreased, and the force of attraction between nucleus and valence electron increased.

27.

Explain why melting and boiling point decreases, going down Group 1.

a)

Metallic bond between atoms becomes weaker, energy required to overcome metallic bond decreased.

b)

Metallic bond between atoms becomes stronger, energy required to overcome metallic bond increased

c)

Metallic bond between atoms becomes stronger, energy required to overcome metallic bond decreased.

d)

Metallic bond between atoms becomes weaker, energy required to overcome metallic bond increased.

28.

When alkali metals are reacted with oxygen gas, metal oxides are produced in form of white solids. Choose the pair that gives the same result and what is it.

a)

Lithium and sodium

b)

Lithium and potassium

c)

Turns green universal indicator into pink

d)

Turns green universal indicator into purple

29.

What can be observed when potassium is reacted with oxygen and chlorine gas?

a)

Burns slowly and produce yellow flame

b)

Burns very brightly and produce purple flame

c)

Burns very brightly and produce yellow flame

d)

Burns slowly and produce purple flame

30.

Magnesium is a Group 2 element. When magnesium carbonate is heated, magnesium oxide is formed and carbon dioxide is liberated.

MgCO3 --> MgO + CO2

Which of the following is true when going down the group?

a)

Lattice energy of carbonates decreases

Lattice energy of oxides decreases

Thermal stabilities of oxide decreases

b)

Lattice energy of carbonates decreases

Lattice energy of oxides decreases

Thermal stabilities of oxide increases

c)

Lattice energy of carbonates increases

Lattice energy of oxides increases

Thermal stabilities of oxide decreases

d)

Lattice energy of carbonates decreases

Lattice energy of oxides increases

Thermal stabilities of oxide decreases

31.

Beryllium is a Group 2 element. Which of the following is the anomalous properties of beryllium?

a)

Beryllium oxide is amphoteric

b)

Beryllium chloride does not dissolve in water

c)

Beryllium forms a covalent compound with fluorine

d)

Beryllium oxide can form dimer.

32.

Steam is passed over heated magnesium to give compound X and hydrogen.


what is not the property of Compound X ?

a)

It has a high melting point

b)

It is a basic oxide

c)

It is a white solid

d)

It is very soluble in water

33.

What can be seen when a piece of magnesium ribbon is placed in cold water?

a)

A vigorous effervescence occurs

b)

Bubbles of gas form slowly on the magnesium

c)

The magnesium floats on the surface of the water and reacts quickly

d)

The magnesium glows and a white solid is produced

34.

When calcium is burnt in oxygen, what colour is the flame?

a)

Green

b)

Red

c)

White

d)

Yellow

35.
Which of the following statements is true about calcium, strontium, and barium?
a)
All the metals liberate hydrogen gas when added to cold water.
b)
All the metal hydroxides are not soluble in water.
c)
All the oxides are amphoteric.
d)
All the metals are stronger reducing agents than Group 1 metals.
36.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
37.
The periodic table is organized by the number of ______ in each element's nucleus
a)
neutrons
b)
protons
c)
electrons
d)
atoms
38.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
39.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
40.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
41.
Which general trends in atomic radius and electronegativity are observed as the elements in Period 3 are considered in order of increasing atomic number?
a)
Atomic radius decreases and electronegativity increases.
b)
Atomic radius increases and electronegativity decreases.
c)
Both atomic radius and electronegativity increase.
d)
Both atomic radius and electronegativity decrease.
42.

Which term represents the strength of the attraction an atom has for the electrons in a chemical bond?

a)

Electrical conductivity

b)

Electronegativity

c)

First ionization energy

d)

Specific heat capacity

43.

Ionic hydrides are formed by

a)

halogens

b)

chalogens

c)

group one elements

44.

Hydrogen is a good (a)   agent

45.

An element Y reacts with cold water. Which of the following is the likely proton number of Y?

a)

4

b)

9

c)

11

d)

15

46.

Why do Group 2 metals have higher m.p than Group 1?

a)

Higher charge and more electrons

b)

Lower charge and less electrons

47.

Which is not a reason that cryolite is used in aluminum extraction?

a)

Cryolite dissolves aluminum oxide

b)

Cryolite reduces the melting point of aluminum oxide

c)

Cryolite decreases the cost of aluminum extraction

d)

Cryolite removes impurities from aluminum oxide

48.

Why can carbon combine with itself to make substances that have very different properties? (ex. graphite and diamond).

a)

Because of carbon's 4 valence electrons it can form a variety of bonds with other carbons.

b)

Because carbon is polar it can combine in a variety of ways.

c)

Because carbon will either give or take 4 electrons so it can form various substances

d)

Because carbon forms cations it combines in various ways.

49.

Which of the following are produced when chlorine is allowed to react with dilute aqueous potassium hydroxide?

a)

H2O(l)

b)

NaOCl(aq)

c)

NaClO3(aq)

d)

KOCl(aq)

50.

Which of the following is the chemical equation for the reaction between chlorine gas and hot aqueous sodium hydroxide?

a)

Cl2(g) + 2NaOH(aq) ----> NaCl(aq) + NaOCl(aq) + H2O(l)

b)

Cl2(aq) + 2NaOH(aq) ----> NaCl(aq) + NaOCl(aq) + H2O(l)

c)

3Cl2(g) + 6NaOH(aq) ----> 5NaCl(aq) + NaClO3(aq) + 3H2O(l)

d)

3Cl2(aq) + 6NaOH(aq) ----> 5NaCl(aq) + NaClO3(aq) + 3H2O(l)

51.

When aqueous silver nitrate is added into a halide solution, a coloured precipitate if formed immediately. This precipitate is insoluble in dilute aqueous ammonia but soluble in both concentrated or excess aqueous ammonia. Name the halide ion present in the halide solution.

(a)  

52.

Among which of the following pairs of the Period 3 elements is the difference in boiling point the greatest?

a)

Silicon and argon

b)

Sodium and argon

c)

Sodium and silicon

d)

Aluminium and chlorine

53.

An oxide of G has a boiling point 2230°C. It dissolves in aqueous sodium hydroxide solution but not in water and acid. Oxide G is

a)

PbO2

b)

P2O5

c)

SiO2

d)

Al2O3

54.

When concentrated sulfuric acid reacts with sodium iodide the products include sulfur, iodine, hydrogen sulfide and sulfur dioxide.

Which statement is correct?

a)

Hydrogen sulfide is the product of a reduction reaction.

b)

Iodide ions are stronger oxidising agents than sulfate ions

c)

Sulfur atoms from the sulfuric acid are both oxidised and reduced.

d)

Sulfur atoms from the sulfuric acid are oxidised to make sulfur dioxide

55.

The electron configuration of chromium in CrO42- ion is

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p63d5

c)

1s2 2s2 2p6 3s2 3p63d5 4s1

d)

1s2 2s2 2p6 3s2 3p6 3d4 4s2

56.

Which of the following element has the highest melting point?

a)

Phosphorus

b)

Silicon

c)

Sulphur

d)

Sodium

57.

Aqueous K𝑋 reacts with aqueous AgNO3 to form a precipitate which does not dissolve in excess ammonia. K𝑋 is

a)

KF

b)

KCl

c)

KBr

d)

KI

58.

Which of the following corresponds to the second ionisation energy of manganese?

a)

Mn+(g) → Mn2+(g) + e

b)

Mn(s) → Mn2+(g) + 2e

c)

Mn+(s) → Mn2+(g) + e

d)

Mn(g) → Mn2+(g) + 2e

59.

Which of the following elements has the highest melting point?

a)

Sodium

b)

Aluminium

c)

Phosphorus

d)

Sulphur

60.

The higher the ionization energy...

a)

the more attracted the valence electron is to the nucleus so it is harder to remove

b)

the less attracted the valence electron is to the nucleus so it is easier to remove

c)

the more attracted the valence electron is to another electron, so it is harder to remove

d)

the more repelled a valence electron is to another electron, so it is easier to remove

61.

The following are basic oxides except for

a)

CuO

b)

BaO

c)

Rb2O

d)

BeO

62.

The following are the properties of ozone except for

a)

It is a pale blue gas

b)

It is a strong reducing agent

c)

It is a polar molecule

d)

It is unstable

63.

Which of the following is not true about sulphur?

a)

It cannot conduct electricity.

b)

It is soluble in water.

c)

It is in the solid state of S8 at room temperature.

d)

It burns with blue flame and emit SO2 gas.

64.

Which of the following is not true about sulphur dioxide, SO2?

a)

SO2 can act as an oxidising agent.

b)

SO2 can act as a reducing agent.

c)

SO2 is released in the combustion of fossil fuels.

d)

SO2 is a basic gas.

65.

The following equation shows one of the reactions occurring in the Contact process:

2SO2(g) + O2(g) ---> 2SO3(g) ∆H = –198 kJ mol-1


The yield of SO3 can be increased by:

a)

Removing SO3 as it forms.

b)

Adding more catalyst.

c)

Increasing the temperature.

d)

Decreasing the pressure.

66.

Choose the correct sequence for the Frasch process.

I. Compressed air is pumped down the center tube.

II. Sulfur slurry is forced out from the middle tube.

III. Superheated steam is forced down the outer tube.

a)

I, II, III

b)

III, I, II

c)

III, II, I

d)

II, III, I

67.

The following are properties of sulphuric acid except for

a)

It is a diprotic acid

b)

It turns red litmus paper to blue

c)

It reacts with metal to form salt and water

d)

salt of H2SO4 can be identified by adding acidified barium chloride solution

68.

SO3 is not allowed to react with H2O directly because

a)

The reaction is highly endothermic

b)

The reaction is slow

c)

The acid produced is diluted

d)

The reaction is violent and creates fog of H2SO4

69.

Ammonia exists as simple covalent molecules, NH3. Ammonia can react with suitable reagents to form products containing ammonium ions, NH4+. Ammonia can also react with suitable reagents to form products containing amide ions, NH2–.

Which of these nitrogen-containing species are present in an aqueous solution of ammonia?

a)

ammonia molecules, ammonium ions and amide ions

b)

ammonia molecules and ammonium ions only

c)

ammonia molecules only

d)

ammonium ions only

70.

Which statement does not describe an effect of acid rain on the environment?

a)

Acid rain causes erosion of stone buildings.

b)

Acid rain causes ozone depletion.

c)

Acid rain increases the corrosion of some metals.

d)

Acid rain increases the leaching away of essential nutrients and minerals from soils.

71.

When concentrated sulfuric acid is added to glucose, a black solid is formed over time. What is the name of the black solid?

a)

Copper(II) oxide

b)

Coal

c)

Carbon

72.

GAS EVOLVED WHEN CARBON REACTS WITH CONC.SULPHURIC ACID

a)

SULPHUR DIOXIDE

b)

CARBON MONOXIDE

c)

HYDROGEN SULPHIDE

73.

DISTINGUISH( CHEMICAL TEST) BETWEEN DILUTE H2SO4 ACID AND DILUTE HNO3 ACID IS DONE BY ADDING---

a)

BARIUM CHLORIDE SOLUTION

b)

BARIUM NITRATE SOLUTION

c)

BARIUM SULPHATE SOLUTION

74.
A piece of filter paper moistened with lead (II) ethanoate solution turns black when the paper is dropped into a gas jar containing an unknown gas. The gas is likely to be
a)
Sulphur (IV) oxide
b)
Hydrogen chloride
c)
Sulphur (VI) oxide
d)
Hydrogen sulphide
75.
Which of the following acts as both a reducing and an oxidizing agent?
a)
H₂
b)
SO₂
c)
H₂S
d)
Cl₂
76.
The solubility of iodine in water is greatly increased by
a)
adding an acid
b)
boiling the solution
c)
cooling the solution
d)
adding potassium iodide
77.
Which pair gives Cl₂ at room temperature?
a)
conc. HCl + KMnO₄
b)
NaCl + conc. H₂SO₄
c)
NaCl+ MnO₂
d)
NaCl + conc. NHO₃
78.
Which of the following arrangements shows increasing order of reactivity of the halogens?
a)
F₂ > Cl₂> Br₂ > I₂
b)
I₂ < Br₂ < Cl₂ <. F₂
c)
F₂ < Cl₂ < Br₂ < I₂
d)
I₂ > Br₂ > Cl₂ > F₂
79.
The bleaching action of chlorine is through the process of
a)
hydrolysis
b)
hydration
c)
oxidation
d)
reduction
80.
On exposure to hydrogen sulphide, moist lead (II) ethanoate paper turns
a)
black
b)
blue
c)
green
d)
yellow
81.
Which of the allotropes of sulphur has amber colour with needle shape?
a)
Rhombic sulphur
b)
Flower suiphur
c)
Monoclinic sulphur
d)
Plastic sulphur
82.
Sulphur(IV) oxide bleaches by
a)
reduction
b)
oxidation
c)
hydration
d)
adsorption
83.

Why is zinc not considered a transition metal?

a)

Zinc is not a transition metal because it gains two 4s electrons to give a 2+ion with full d subshell levels.

b)

Zinc is not a transition metal because it loses four 4s electrons to give a 4+ion with full d subshell levels.

c)

Zinc is not a transition metal because it loses two 4s electrons to give a 2+ion with full d subshell levels.

d)

Zinc is not a transition metal because it gains two 4d electrons to give a 2+ion with full d subshell levels.

84.

Which of the following properties about transition elements is incorrect?

a)

Transition metals have variable oxidation state.

b)

They are the only elements that can form coloured ions in aqueous solution.

c)

Transition elements are good catalyst.

d)

They are the only elements that can form complexes.

85.

Cobalt has a proton number of 27. Choose the correct electronic configuration for Co4+.

a)

[Ar]3d34s2

b)

[Ar]3d7

c)

[Ar]3d74s2

d)

[Ar]3d5

86.

Which of the transition elements exhibit highest oxidation state?

a)

Manganese

b)

Vanadium

c)

Iron

d)

Chromium

87.

When excess ammonia is added to aqueous Cu2+ ion, a complex ion of [Cu(NH3)4]2+ is formed. Which of the following statements is true about the reaction above?

a)

Ammonia acts as a Lewis base.

b)

[Cu(NH3)4]2+ is not stable.

c)

Ammonia is a stronger ligand than water.

d)

Cu2+ is a stable ion.

88.

During the complex formation,

a)

the metal cation and the ligand share one electron each.

b)

the metal cation accepts two electrons from the ligand.

c)

two electrons from the metal are transferred to the ligand.

d)

the metal cation donates both its d electrons to the ligand.

89.

Arrange the melting point of manganese, magnesium and potassium in increasing order.

a)

K<Mg<Mn

b)

Mn<K<Mg

c)

Mn<Mg<K

d)

Mg<Mn<K

90.

Which of the following properties about transition elements is incorrect?

a)

Transition metals have variable oxidation state.

b)

They are the only elements that can form coloured ions in aqueous solution.

c)

Transition elements are good catalyst.

d)

They are the only elements that can form complexes.

91.

1. Glass is made up of ___________.

a)

aluminium silicate

b)

silica

c)

brass

d)

pewter

92.

Monoxides and dioxides of Group 14 elements in the Periodic Table show different acid-base properties. Which is an acidic oxide?

a)

GeO

b)

PbO

c)

SiO2

d)

SnO2

93.

a)

A

b)

B

c)

C

d)

D

94.

a)

A

b)

B

c)

C

d)

D

95.

When compound X is heated, it changes colour from green to black. Compound Y is formed and a gas is given off which turns limewater milky.

X and Y are ......................................, respectively.

a)

calcium carbonate and calcium oxide

b)

copper carbonate and carbon

c)

copper carbonate and copper oxide

d)

copper sulfate and copper oxide

96.

Two industrial processes that involve heating are

1. extracting iron from its ore using a blast furnace

2. making lime.

In which of these processes is calcium carbonate used?

a)

Process 1

b)

Process 2

c)

Both 2 processes

d)

None of the processes

97.

What leaves the furnace at X?

(a)  

98.

When sodium hydroxide solution is added to the Iron(III) solution until excess

a)

A brown solution is formed

b)

A brown precipitate is formed

c)

A green precipitate is formed

d)

A green solution is formed

99.

Below here are examples of reducing agent except

a)

Magnesium

b)

Sulphur dioxide

c)

Hydrogen sulphide

d)

Chlorine water

100.

A few drops of sodium hydroxide solution was added to a metal salt solution.

A dark green gelatinous precipitate was formed.

Which metal ion (cation) was present in the salt solution?

a)

iron(III) ion, Fe3+

b)

iron(II) ion, Fe2+

c)

copper(II) ion, Cu2+

d)

zinc ion, Zn2+

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9th - 12th Grade

Chemistry- Final Exam Review

105 questions

Chemistry- Final Exam Review

quiz

Worksheet

•

9th - 12th Grade