Name………………………………………………………………….
Period …….
Regents Review 3: Bonding
Review Book: Topic 6
BONDING – REFER TO UNIT 6 NOTES FOR MORE INFORMATION (RULES FOR DRAWING ELECTRON-DOT STRUCTURES)

WHY DO ELEMENTS BOND (STICK TOGETHER)?
to get a COMPLETE (STABLE) VALENCE SHELL – an OCTET of ELECTRONS

HOW DO ELEMENTS BOND (STICK TOGETHER)?
Nonmetals:
1 atoms share electrons (COVALENT BONDS)
Metals and
Nonmetals:
2 atoms lose/gain electrons and form ions (IONIC BONDS)
Metals only:
3 atoms “float” in a “sea” of mobile electrons (METALLIC BONDS)
SUMMARY: PROPERTIES OF METALLIC, IONIC, AND COVALENT SUBSTANCES
TYPE OF
TYPE OF SUBSTANCE
METALLIC SUBSTANCE
(METAL)
ex: Ca, Co, K, Na
BOND IN
SUBSTANCE
METALLIC
(e–s are
transferred
from metal to
nonmetal)
ELECTRICAL
HARDNESS
CONDUCTIVITY?
SOLID LIQUID AQUEOUS
MALLEABLE
(BENDABLE)
(sea of mobile
e–s)
IONIC
IONIC COMPOUND
ex: NaCl, CaCO3, Mg(OH)2
MELTING
& BOILING
POINTS
YES!
HIGH
BRITTLE &
HARD
NO
YES!
(ELECTROLYTES)
COVALENT (MOLECULAR)
COMPOUND
ex: CO2, NH3, CH4, CH3OH
COVALENT NETWORK SOLID
ex: diamond (C),
silicon dioxide (SiO2)
NONPOLAR or
POLAR
LOW
SOFT
NO
COVALENT
(e–s are shared)
VERY HIGH
VERY HARD
***HYDROGEN BONDS*** are a special kind of bond between MOLECULES that contain H bonded to F, O, or
N atoms. Hydrogen bonds are a strong INTERMOLECULAR force which cause substances like water to have
high melting and boiling points.
1. Which of the following is the correct electron dot
diagram for nitrogen?
2. In water, the bond between hydrogen and oxygen is
(1) ionic
(2) polar covalent
(3) nonpolar covalent
(4) metallic
3. The bonds in MgSO4 can be described as
(1) both ionic and covalent
(2) ionic, only
(3) covalent, only
(4) ionic and covalent
7. The formula for magnesium fluoride is MgF2. The
best explanation for this fact is that when they
combine
(1) each of two magnesium atoms lose an electron
and a fluorine atom gains two
(2) a magnesium atom loses two electrons and each
of two fluorine atoms gains one
(3) a magnesium atom shares two electrons with two
fluorine atoms
(4) each of two magnesium atoms share an electron
with a fluorine atom
8. When calcium combines with a nonmetal, it usually
(1) loses two electrons
(2) gains six electrons
(3) shares two electrons
(4) shares six electrons
9. Which substance will conduct electricity in both the
solid phase and the liquid phase?
(1) AgCl (2) H2 (3) Ag (4)HCl
4. Which of the following occurs during covalent
bonding?
(1) Electrons are lost.
(2) Electrons are gained.
(3) Valence electrons fall from the excited state to
the ground state.
(4) Unpaired electrons form pairs.
5. Which of the following is an example of a substance
with a nonpolar covalent bond?
(1) HCl
(2) Cl2
(3) HClO2
(4) NaCl
10. Hydrogen bonds are strongest between molecules of
(1) HBr(g) (2) HF(g) (3) HI(g)
(4) HCl(g)
11. The strongest hydrogen bonds are formed between
molecules of
(1) H2Te (3) H2O
(2) H2Se (4) H2S
12. What type of bonds are present in a strip of
magnesium ribbon?
(1) covalent
(2) metallic
(3) ionic
(4) hydrogen bonds
13. Hydrogen bonds are most likely to exist between
molecules of
(1) H2
(2) HI
(3) CH4
(4) H2O
6. Which molecule is polar?
(1) H2
(2) CH4
(3) N2
(4) HCl
14. Which substance, in the solid state, is the best
conductor ofelectricity?
(1) Ag
(2) NaCl
(3) I2
(4) CO2
15. Which is the predominate type of attraction between
molecules of HF in the liquid state?
(1) hydrogen bonding
(3) metallic bonding
(2) ionic bonding
(4) covalent bonding
16. Which substance exists as network of covalent
bonds?
(1) Ar
(2) Au
(3) SiO2
(4) CO2
17. Mobile electrons are a distinguishing characteristic
of
(1) an ionic bond
(3) an electrovalent bond
(2) a metallic bond
(4) a covalent bond
18. What kind of bonds are found in a sample of
H2O(s)?
(1) hydrogen bonds, only
(2) covalent bonds, only
(3) both ionic and hydrogen bonds
(4) both covalent and hydrogen bonds
19. Which substance is made up of molecules that are
polar?
(1) N2 (2) CH4 (3) H2O (4) CO2
20. Which element consists of positive ions immersed in
a "sea" of mobile electrons.?
(1) sulfur (2) calcium (3) nitrogen (4) chlorine
21. Which compound contains ionic bonds?
(1) CaO
(3) SiO2
(2) NO
(4) CO2
22. Which of the following solids has the highest
melting point?
(1) Na2O
(3) SO2
(2) H2O
(4) CO2
23. Which molecule is nonpolar?
(1) CO2
(3) CO
(2) H2O
(4) NH3
24. Which substance contains metallic bonds?
(1) Hg (l)
(3) H2O (l)
(2) NaCl (s)
(4) C6H12O6 (s)
25. Explain, in terms of valence electrons, why the bonding in barium oxide, BaO, is similar to the bonding in magnesium
fluoride, MgF2.
26. Draw the Lewis electron-dot structure for the compound magnesium fluoride.
27. Explain, in terms of valence electrons, why the bonding in fluorine, F2, is similar to the bonding in chlorine, Cl2.
28. Draw the Lewis electron-dot structure for fluorine, F2.
Questions 29 through 32 refer to the following:
Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are
bonded together.
Molecule A:
Cl2
Molecule B:
CCl4
Molecule C:
NH3
29. Draw the electron-dot (Lewis) structure for the NH3 molecule in the box below.
30. Explain why CCl4 is classified as a nonpolar molecule.
31. Explain why NH3 has stronger intermolecular forces of attraction than Cl2.
32. Explain how the bonding in KCl is different from the bonding in molecules A, B, and C.
Questions 33 through refer to the following.
Nitrogen and carbon dioxide are gases present in the atmosphere.
33. Draw the electron-dot diagram for a molecule of nitrogen, N2.
34. Draw the electron-dot diagram for a molecule of carbon dioxide, CO2.
35. What is the total number of electron pairs shared between the nitrogen atoms in a molecule of nitrogen, N2? ______
36. State one similarity and one difference between the bonding within a molecule of nitrogen and the bonding within a
molecule of carbon dioxide.