WorksheetsTypes of Bonding in Crystalline Solids
Total questions: 55
Worksheet time: 28mins
Which type of crystalline solid consists of atoms or molecules and is held together by London dispersion forces, dipole-dipole forces, and hydrogen bonds?
Molecular
Covalent-network
Ionic
Metallic
What type of bonding is present in covalent-network solids?
Metallic bonds
Covalent bonds
Electrostatic attractions
Hydrogen bonds
Fill in the blank: Ionic solids are composed of (a) and are held together by electrostatic attractions.
Which type of solid is described as soft to very hard, with low to very high melting point, excellent thermal and electrical conduction, malleable and ductile?
Molecular
Covalent-network
Ionic
Metallic
Covalent-network solids generally have poor thermal and electrical conduction.
True
False
Fill in the blank: The property of being hard and brittle with high melting point and poor thermal and electrical conduction is characteristic of (a) solids.
Molecular structures consist of (a) molecules.
Atoms in the molecules are held by which type of bonds?
Weak covalent bonds
Strong covalent bonds
Ionic bonds
Metallic bonds
Molecules are held together by weak intermolecular forces. Which of the following is NOT an example of an intermolecular force?
Dipole-dipole forces
London dispersion forces
Hydrogen bonds
Covalent bonds
There are two types of molecular structures: _______ and _______.
(a)
Atoms in the molecules are held by weak covalent bonds.
True
False
Substances with simple molecular structures may be solids, liquids or gases at room conditions. Which of the following is true about substances with simple molecular structures at room conditions?
They are always solids
They can be solids, liquids, or gases
They are always liquids
They are always gases
Substances with macromolecular structures are always solids at room conditions.
True
False
Giant structures are classified into how many types?
2
3
4
5
Which of the following is NOT a type of giant structure?
Giant covalent
Giant ionic
Giant metallic
Giant molecular
What governs the physical properties of molecular solids?
Ionic bonds
Covalent bonds
van der Waals forces
Metallic bonds
Fill in the blank: The individual units of molecular solids are (a) molecules.
Which of the following is a property of simple molecular substances?
High melting points
Low melting points and boiling points
Conductors of electricity
Insoluble in non-polar solvents
Are simple molecular substances conductors of electricity?
Yes
No
Simple molecular substances are usually insoluble in polar solvents but soluble in (a) solvents.
What principle explains the solubility of simple molecular substances in non-polar solvents?
Opposites attract
Like dissolves like
High melting point
Conductivity
What are macromolecules?
Short chains of molecules containing a small number of atoms
Long chains of molecules containing a very large number of atoms
Single molecules with a few atoms
Molecules with no atoms
Which of the following is an example of a macromolecule?
Water
Plastics
Oxygen
Sodium chloride
Macromolecules have higher m.p./b.p. than simple molecules due to much stronger ________ forces.
Van der Waals'
Ionic
Covalent
Hydrogen Bond
Which of the following best describes giant covalent substances?
Non-metallic atoms are joined together by strong covalent bonds in large networks or chains
Metallic atoms are joined together by ionic bonds
Non-metallic atoms are joined together by weak bonds in small molecules
Metallic atoms are joined together by metallic bonds
Are discrete molecules present in giant covalent substances?
True
False
Which is an example of giant covalent substances?
diamond, graphite, and quartz
Lead, diamond and graphite
Copper, diamond, lead
Graphite, quartz, copper
Which of the following is NOT an example of a giant covalent substance?
A) Diamond
B) Graphite
C) Quartz
D) Sodium chloride
Graphite is a good conductor of electricity because the unhybridized π electrons of carbon atoms are (a) within the layers.
What type of attraction holds cations and anions together in ionic substances?
Weak directional covalent attraction
Strong non-directional electrostatic attraction
Weak non-directional electrostatic attraction
Strong directional covalent attraction
Fill in the blank: Oppositely charged ions are closely packed together to give a 3-dimensional (a) .
What is the reason ionic compounds tend to be hard and have high melting point solids?
Ionic bonds are weak and flexible
Ionic bonds are strong and rigid
Ionic bonds are metallic
Ionic bonds are covalent
Why do ionic solids generally not conduct electricity in solid state?
Ions are free to move
Ions are held in a rigid ionic lattice
There are delocalised electrons
They dissolve in water
What type of character may ionic bonds have if the cation is small and/or highly charged?
Metallic character
Covalent character
Ionic character
Hydrogen bonding
Which cation among Na⁺, Mg²⁺, and Al³⁺ has the highest polarizing power?
Na⁺
Mg²⁺
Al³⁺
Which anion paired with Al³⁺ will have the most distorted electron cloud?
F⁻
Cl⁻
Br⁻
The polarizability of the anion depends on which of the following?
Size and charge
Temperature and charge
Size and shape
Mass, size and charge
For anions having the same charge, which anion is polarized to a greater extent?
Smaller anion
Larger anion
Anion with higher charge density
Anion with lower charge density
What do metallic substances consist of?
Regular lattice of metallic cations and a 'sea' of delocalized electrons
Regular lattice of non-metallic anions and localized electrons
Random arrangement of atoms
Only metallic cations
In metals, valence electrons are _______ throughout the solid.
rigidly bonded
localized
emitted
What is a property of metallic substances? Fill in the blank: Metallic substances are good conductors of ______ and ______.
heat, light
electricity, charge
charge, heat
Which of the following is a property of giant covalent substances?
Low melting points and boiling points
High melting points and boiling points
Soluble in water
Good conductors of electricity
Which of the following describes the conductivity of giant covalent substances?
Good conductors of heat and electricity
Poor conductors of heat and electricity
Conductors only in molten state
Conductors only in solution
Which of the following is NOT a property of ionic substances?
High melting and boiling points
Hard but brittle
Low melting and boiling points
Hard and flexible
The giant ionic structure fractures when a stress is applied.
True
False
What property of metals allows electrons to move freely and carry electric current?
Ductility
Conductivity
Hardness
Metallic lustre
Which metal is the best electrically conducting metal?
Copper
Lead
Aluminum
Which of the following statements is true about the density of metals?
Metals have low density because their atoms are loosely packed.
Metals have high density because their atoms are closely packed.
Metals have low melting points.
Lithium is the densest metal.
Which of the following is an example of an ionic compound?
NaCl
H2O
SiO2
Fe
Fill in the blank: Covalent bonds hold all the atoms or molecules together in a (a) molecular structure, e.g. diamond (C), quartz (SiO2), silicon (Si), silicon carbide (SiC).
What type of intermolecular force is present in H2O, NH3, and HF?
van der Waal's
Permanent dipole-permanent dipole
Hydrogen bonds
Ionic bonds
Which of the following elements has the highest boiling point?
Sodium
Magnesium
Aluminium
Silicon forms giant covalent molecules in which each Si atom is covalently bonded to how many other Si atoms?
2
3
4
5
White phosphorous is described as a white waxy solid. What type of intermolecular forces hold the P4 molecules together?
Strong covalent bonds
Weak van der Waal’s forces
Strong van der Waal’s forces
Weak covalent bonds
Sulphur typically forms S8 molecules held together by instantaneous-induced dipole attractions. Compared to P4, what is S8's boiling point?
Higher
Lower
The same
Not enough information to tell
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