Worksheetssec 2 lesson 4
Total questions: 20
Worksheet time: 3600secs
What is the number of the lone pairs of electrons on arsenic atom 33As in arsine AsH3?...............
Zero
1
2
3
The opposite figure represents a/an …………… compounds.
ionic
polar covalent
pure covalent
acidic
The covalent bonding in methane molecule CH4 requires …………… electrons.
10
8
4
2
According to VSEPR, the presence of 4 bond pairs of electrons around the central atom causes the molecule to have the stereostructure.
linear
planar triangle
angular
tetrahedron
Which of these statements explains why atoms of neon do not form ionic bonds?
Atoms of neon have delocalised electrons
Atoms of neon must gain or lose four electrons to form a stable octet in their outer shell
Atoms of neon already have a stable octet in their outer shell.
Which of the following pairs of compounds are similar in their molecular Stereostructure?
BF3 , NH3
BeCl2 , H2O
CCl4 , CH4
PF3 ,IF3
Which of the following compounds molecules contains 2 bond pairs and 2 lone pairs of electrons?
NH3
SO2
H2S
BF3
The opposite graphical figure illustrates the melting points of different elements, among which is sodium , which of the illustrated Setters represents sodium element?
A
B
C
D
Three students assumed three factors which affect the strength of the hydrogen bond:
Factor (1): The angle between the hydrogen bond polar bond in the same molecule.
Factor (2): The number of bond pairs of electrons in the central atom.
Factor (3): Difference in electronegativity between the hydrogen atom and the other atom binded to it.
Which of these factors are correct? ...............
(1) , (2)
(1) , (3)
(2) , (3)
(1) , (2) and (3)
Molecules of HF , H2O and NH3 are all able to form hydrogen bonds.
What property of a molecule gives it the ability to form a hydrogen bond?
A large difference in electronegativity between hydrogen and the atom it is bonded to
The number of hydrogen atoms covalently bonded to an atom of a different element
The ability to conduct electricity in aqueous solutions
The electronegativities of nitrogen (3.04) and bromine (2.96) are very similar; however, nitrogen has a much greater ability to form hydrogen bonds than bromine. How can this difference in hydrogen-bonding ability be rationalized?
An atom of bromine contains more protons in its nucleus and so attracts an atom of hydrogen strongly enough to form covalent bonds instead of hydrogen bonds.
The larger size of a bromine atom means it forms weaker bonds to hydrogen and so does not form strong hydrogen bonds.
An atom of nitrogen contains more lone pairs than an atom of bromine, giving it a greater ability to form hydrogen bonds.
Hydrogen bonds are found between the molecules of all the following compounds, except on.
HF
NH3
HCL
H2O
There are …………... bonds in a sample of water.
only Hydrogen
only ionic
only covalent
covalent and hydrogen
Which of the following molecules contains 6 bond electrons?...............
C2H4
H2S
NCl3
SF6
The bond between fluorine and oxygen is relatively weak because of ……………
the repulsion forces between the lone pairs of electrons in the atom of each of them.
the large atomic radius of oxygen
the ionic bonding between them.
In CS2 molecule, the central carbon atom binds to each of the two sulphur atoms with ……………
1 σ bond and 1 π bond.
2 π bond.
2 σ bond.
Ionic bond originates between ……………
a cation of a nonmetal and an anion of a metal.
a metal with large atomic size and a nonmetal with high electron affinity.
two metals have the same electronic configuration.
Which of the following orbitals in carbon its electrons do not participate in forming C–C bond in ethane molecule C2H6?...............
1s only
2s only.
2p only.
1s and 2s
Which of these choices includes a pair of compounds or ions which contain both covalent bonds and coordinate bonds?...............
NH3,NH4
PH4,H3O
H3O,H2O
H2O,HCL
The opposite figure represents the arrangement of ions in a crystal lattice, what is the expected value of the difference in the electronegativity between the anion and the cation which form this crystal lattice?...............
0.5
0.9
1
2.1
