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Worksheetssec 2 lesson 3 chapter 3
Total questions: 20
Worksheet time: 3600secs
In the structural formula of the opposite compound:What are the number of the valence electrons of the elements of this compound which do not participate in forming the bonds?...............
6
8
10
12
The Lewis structure for an atom of helium is shown below. Which of these statements explains why helium does not usually form chemical bonds?
The first electron shell can hold eight electrons, but finding six electrons for a full valence shell is too difficult.
The first electron shell can only hold two electrons; therefore, helium has a full valence shell.
Helium is a gas and therefore cannot lose its two electrons.
The Lewis structure for a molecular compound of potassium and sulfur is shown below. How can you tell this compound is ionically bonded?
Ionic compounds always contain atoms in a 2 : 1 ratio.
The atoms are sharing electrons to obtain full outer shells but have not become ions.
The atoms have either lost or gained electrons to become ions and obtain full outer shells.
The molecule …………… includes three bond pairs.
HBr
H2O
NF3
O2
In which of the following compounds the ionic character predominates?...............
CH3Cl
CH4
Cl2
RbCl
Which of the following values represents the difference in electronegativity in a good electric conducting compound? ……………
0.4
1.2
1.5
2.1
The structures of most compounds can be classified as simple molecular, giant covalent, ionic, or metallic. All but one of the following compounds exhibit the same type of structure. For which compound is a different type of structure observed?
MgBr2
NaCl
CH4
An ionic compound is made from a metal,M and a nonmetal, X .The electron dot diagrams for M and X are shown below. Which of the following molecular formulas will the ionic compound have?
M2X3
M2X
MX
MX3
Which of the following accounts for the high melting point of ionic compounds?
The electrostatic force of attraction between the oppositely charged ions
Hydrogen bonding between negative and positive poles
The forces that arise from sharing a pair of electrons
Why do ionic compounds conduct electricity in molten and aqueous phases but not in the solid phase?
The ions are free to move in aqueous and molten phases but not in the solid phase.
The electrons are free to move in aqueous and molten phases but not in the solid phase
Bonds in solid ionic compounds are nonpolar, while bonds in molten and aqueous ones are polar.
What is the regular arrangement of ions in an ionic structure called?
A giant covalent structure
A crystal lattice
An amorphous solid
What force holds ionic structures together?
Metallic bonds
Magnetism
Electrostatic attraction
Which of these statements does not describe a difference between covalent and ionic compounds?
Covalent compounds have low melting and boiling points.
Covalent compounds are bonded through electrostatic attraction.
Ionic compounds can conduct electricity when dissolved or melted
Why do covalent compounds have lower melting and boiling points compared with ionic compounds?
Covalent compounds do not conduct electricity.
Covalent compounds have weak intermolecular forces between the molecules.
Covalent compounds do not form between metals and nonmetals.
Covalent compounds have very weak bonds between the atoms.
Which of the following is the number of covalent bonds that can be formed by an unbound atom of carbon? Carbon can be found in group 14 of the Periodic Table.
8 bonds
4 bonds
3 bonds
In a Lewis diagram, how many dots would be placed around a boron atom? This element can be found in group 13 of the Periodic Table.
2 dots
8 dots
3 dots
Which of the following is displayed in a Lewis dot diagram?
The valence protons in an element
The valence electrons in an element
The electrons in the last 2 shells in an element
Which of the following defines the octet rule?
A rule that refers to the tendency of an atom to have empty valence shells
A rule that refers to the tendency of an atom to have 8 electrons in the valence shell
A rule that refers to the tendency of electrons to orbit around an atom in energy shells
Which of the following pairs of elements is likely to bond covalently?
Mg and Cl
Fe and H
P and F
Which of the following compounds is the most covalent?
GeCl4
LaCl3
CCl4
