Miss Licata
1/6/09
Cp-Chemistry
Chapter 6 Study Guide
6-1
1. Definition of a chemical bond –
2. Ionic bonding results from the electrical attraction between large numbers of
________________ (+ ions) and ________________(- ions)
3. Covalent bonding results from the _______________ of electron pairs between 2
atoms
4. In ionic bonding there is ____________differences in electronegativity values
between atoms.
5. The Δ electronegativity > 1.7 for which of the following
a.
b.
c.
d.
covalent
nonpolar covalent
ionic
neutral atoms
6. Nonpolar covalent bonding electrons are shared_______________ by the bonded
atoms, resulting in a balanced distribution of electrical charge
7.
The Δ electronegativity: 0 to 0.3 (roughly) for which of the following:
a.
b.
c.
d.
covalent
nonpolar covalent
ionic
neutral atoms
8. Polar covalent bonding electrons are shared ______________because one atom
pulls, although not very strongly, more on the electron pair than the other atom
9. The Δ electronegativity: 0.3 to 1.7 for which of the following:
a. Polar covalent
b. nonpolar covalent
c. ionic
d. neutral atoms
10. Determine the electronegativity differences, the probable bond type, and the more
electronegative atom with respect to bonds formed between the following pairs of
atoms (page 151)
Zn and O
Br and I
S and Cl
6-2 Covalent bonding
11. As atoms approach, ________________ increases and potential E
goes___________ Beyond a certain point, _____________ increases and E goes
__________
12. Definition of a molecule –
13. molecular compound is
a.
b.
c.
d.
a compound that is made of molecules
shows the kinds & #s of atoms making up a molecule
molecule containing only 2 atoms
neutral group of atoms held together by covalent bonds
14. Diatomic molecule is
a. a compound that is made of molecules
b. shows the kinds & #s of atoms making up a molecule
c. molecule containing only 2 atoms
d. neutral group of atoms held together by covalent bonds
15. Molecular formula is
a. a compound that is made of molecules
b. shows the kinds & #s of atoms making up a molecule
c. molecule containing only 2 atoms
d. neutral group of atoms held together by covalent bonds
16. Bond Length: average______________ between 2 bonded atoms
17. Energy required to break a chemical bond and form neutral isolated atoms is
called _________________
18. Chemical compounds tend to form so that each atom, by gaining, losing or
sharing electrons, has an_______________of electrons in its highest (outermost)
energy level
19. Electron configuration notation in which only the valence electrons of an atom of
a particular element are shown, indicated by ___________ placed around the
element’s ____________
20. Write the electron-dot notation for each of the following elements:
a.
He
b.
O
c.
B
21. Draw the Lewis structure for each of the following molecules
a.
CCl2F2
b.
CH3NH2
22. Draw the Lewis structure of the following:
N2
23. Draw the resonance structures of the following polyatomic ion
H3C2O2-
24. Draw the Lewis structure of the following polyatomic ions
OHBrO3-
6-3 Ionic bonding
25.________________________ composed of positive and negative ions that are
combined so that the number of positive charges are equal to (cancel out) the number of
negative charges
26. Ions reach a lower potential E through the electrical forces of attraction between
oppositely charged particles when they combine in an orderly arrangement known as a
_________________________
27. Covalent bonding: simplest unit is a_______________ Ionic bonding: simplest unit
is a ________________
28. Term used to describe bond strength in ionic compounds
a.
b.
c.
d.
bond strength
lattice energy
bond energy
energy
29. Energy________________when one mole of an ionic crystalline compound is formed
from gaseous ions
30. Review the Ionic verses covalent bonding properties (notes) including conductivity
and hardness/brittleness
31. A charged group of covalently bonded atoms is are__________________
32. ________________bonding consists of metals that have very few electrons in their
highest E level
33. “delocalized electrons” _______________don’t stay in one locality like…
– covalent bonding: stay in the overlapping of the _______ orbitals
– ionic bonding: e-s are bound to an ion within a ______________
34. The chemical bonding that results from the attraction between metal atoms and the
surrounding sea of electrons
a. covalent bonding
b. ionic bonding
c. metallic bonding
d. polar covalent bonding
35. Know the why metals are:
 good electrical conductors
 good thermal conductors
 shiny
 malleable/ductile