Transcript Practice Quiz

Practice Quiz
Ionic and Covalent
Bonding
Remember….these are our targets (so far)…
• Describe how one can identify a compound as ionic or molecular.
• Explain the role and location of electrons in a covalent bond.
• Describe the change in energy and stability that takes place when a
covalent bond forms.
• Explain the difference in single, double and triple covalent bonds.
• Distinguish between polar and non-polar covalent bonds based on
electronegativity differences.
• Contrast ionic and molecular substances in terms of their physical
characteristics and the types of forces that govern their behavior.
• Show the process of how an ionic bond forms.
• Explain how properties of ionic compounds depend on the nature
of ionic bonds.
• Describe the formation of a salt.
• Draw Lewis Dot diagrams (electron dot diagrams) of elements.
• Rationalize the properties of a substance based on its type of
bonding.
The element represented by
2
10
2
[Ar] 4s 3d 4p
Is which element?
a. Titanium
b. Silicon
c. Germanium
d. Selenium
Has how many valence
electrons?
a. 2
b. 4
c. 10
d. 12
e. 14
The element represented by
[He] 2s2 2p4
Would need to share how many electrons with
another atom to achieve a noble gas
configuration?
a. 2
b. 4
c. 6
d. 8
e. None of these are correct.
Use the electron dot diagrams to
answer the following question
Which combination of elements would likely form a
covalent bond?
a. V and X
b. V and Z
c. W and Y
d. W and Z
e. Y and Z
If two atoms (X and Z) were to
covalently bond to each other, what
molecule would result?
a.
b.
c.
d.
e.
XZ
X2Z3
X3Z
XZ3
It is impossible to answer because atoms of X
will not covalently bond .
If two atoms of Y could covalently
bond together, what type of bond
would result?
a.
b.
c.
d.
e.
a single, polar bond
a double, nonpolar bond
a triple, polar bond
a single, nonpolar bond
It is impossible to answer because two
atoms of Y will not covalently bond.
Which of the following compounds
could be created by ionic bonding?
a.
b.
c.
d.
e.
VZ
WY
XZ3
YZ2
None of These
Of the electron dots structures below,
which would represent an atom of
Sulfur?
a. V
b.
c.
d.
e.
W
X
Y
Z
Which of the electron dots
would represent a metal atom?
a. V
b.W
c. X
d.Y
e.Z
Covalent bonding normally occurs
between which types of elements?
a.
b.
c.
d.
e.
metals only
non-metals only
metals and non-metals
More than one of these are correct.
None of these are correct.
Of the three major types of bonding
(ionic, covalent, metallic) which ones are
based on electrostatic attractions
between opposite charges?
A)only ionic bonding
B)only ionic and covalent bonding
C)only ionic and metallic bonding
D)ionic, covalent and metallic bonding
E)none of the above
Ionic compounds normally
conduct electricity
A)when in the solid state.
B)only when molten.
C)when in aqueous solution or molten.
D)only when in aqueous solution.
E)when a solid or in aqueous solution.
Order the following by decreasing
bond length: C≡C, C=C, C-C
A) they are all the same
B) C≡C, C=C, C-C
C) C≡C, C-C, C=C
D) C-C, C=C, C≡C
E) C=C, C-C, C≡C
If a process in salt formation is
exothermic, when we write an
equation, where would “energy”
appear?
a.
b.
c.
d.
e.
On the left side of the arrow
On the right side of the arrow
On top of the arrow
On the reactants side
On the products side
Which selection below is an
endothermic reaction that occurs
in the formation of a salt?
a.
b.
c.
d.
Na + energy  Na+ + eNa + e-  Na+ + energy
Cl + energy  Cl- + energy
Cl + e-  Cl- + energy
Which of the following is NOT a
process in the formation of a salt?
a.
b.
c.
d.
Na + energy  Na+ + eNa(s) + energy  Na(g)
Na+ + Cl-  NaCl + energy
Cl + energy  Cl- + e-
Electronegativity is a measure of
A) the energy needed to remove an electron from an
atom.
B) the energy released when an electron is added to an
atom.
C) the magnitude of the negative charge on an electron.
D) the attraction by an atom for electrons in a chemical
bond.
E) the magnitude of the negative charge on a molecule.
Which of the following elements is
the most electronegative?
A) C
B) Si
C) As
D) Cl
E) Sr
Consider an isolated H-C bond in an organic
compound. Based on the electronegativities of
the two elements, which of the following best
describes the net charge on the carbon atom?
A) no polarization of the bond, i.e. no net charge
B) a full negative charge
C) a full positive charge
D) a partial negative charge
E) a partial positive charge
Which one of the following
properties is not characteristic of
typical metals?
A) moderately high melting point
B) high boiling point
C) brittleness
D) good electrical conductor when solid
E) good electrical conductor when molten
When an atom loses an electron, it
A. becomes a negative ion
B. becomes a positive ion
C. forms a covalent bond
D. gains protons
E. becomes a neutral atom
Which of these is a property of an
ionic compound?
A. Low melting point
B. Poor conductor of electricity
C. Crystal shape
D. Shared electrons
E. Forms a molecule
Ionic compounds have
A. a positive charge
B. a negative charge
C. no electrical charge
D. a changing electrical charge
E. a variable electrical charge depending on the
ions involved
What kind of bond is each picture showing?
Answer…
Covalent Bonds!
Which of the above diagrams is showing a
molecule made of double bonds?
Answer…
Which is showing
a molecule made
of POLAR bonds?
Answer…
The diagram below is showing what?
Answer… The energy changes that occur as a
covalent bond forms.
A
A
B
B
Which part of the diagram is showing
when a molecule
is most stable?
C
D
Answer…
B
B
This is when the
bond is at its lowest
energy!!!
The octet rule helps predict the
number of electrons an atom will
gain or lose
True
or
False
Ionic substances are usually soft
and have a low melting point.
True
or
False
So what are some characteristics of
ionic substances?
Are you a bonding
?