5.1 Atoms, Bonding and the Periodic Table
Guided reading and Study
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
Valence
True
Hydrogen, 1 Carbon , 4 Oxygen, 6
D
True
Atomic number
Period
+1,+2,+3, +/-4, -3,-2-1,0
Lose e- to Gain e8
1,2,3,4,3,2,1,0
Family or Group
Valence electron
A. alkali metals b. high c. halogen d. high e. noble gas f. low
Lost, gained or shared
High to low
Valence electrons = 4,5,6,7,8
Gain and share eSome form ionic bonds and lose e-/ some form covalent bonds and share e1
false
5.2 Ionic Bonds
Guided Reading and Study
Use Target Reading Skills
Sample questions and answers:
Formation of an Ionic Bond
Q. What is an ionic bond?
A. An ionic bond is the attraction between two
oppositely charged ions.
Q. What is the overall charge on an ionic
compound?
A. Overall, an ionic compound is electrically
neutral.
1. ion
2. It loses a negative charge and becomes a
positive ion.
3. It gains a negative charge and becomes a
negative ion.
4. polyatomic ions
5. a. 1+ b. Na+ c. 2+ d. Mg2+ e. 1f. Cl
g. 2h. SO4
2
6. two more electrons than protons; its charge
is 2
7. A sodium atom becomes a positive ion, and
a chlorine atom becomes a negative ion.
8. An ionic bond is the attraction between two
oppositely charged ions.
9. Accept any answer that names one of the
positive ions and one of the negative ions from
the table.
10. chemical formula
11. True
12. The number “2” is called a subscript. It tells
you that there are two chloride ions for each
magnesium ion in the compound.
13. False
14. When the negative ion is a single element
15. hard, brittle crystal structures, high melting
points, ability to conduct electricity in solution
or when melted
16. crystal
17. Every ion is attracted to ions of opposite
charge that surround it.
18. Because ionic bonds are strong, and a lot of
energy is needed to break them
19. solids
20. The ions in solid crystals are tightly bound
to each other, so no energy can flow. When ionic
compounds are dissolved in water, the bonds
between ions are broken, allowing the ions to
move freely and conduct electricity.
Atoms and Bonding
5.3 Covalent Bonds
Guided Reading and Study
Use Target Reading Skills
Possible questions and answers:
How do covalent bonds form?
(Covalent bonds
form when two atoms share electrons.)
What are molecular compounds?
(Molecular
compounds are compounds that consist of molecules
bonded with covalent bonds.)
How does unequal sharing of electrons affect
the atoms in molecular compounds?
(Unequal
sharing of electrons causes the bonded atoms to have
slight electrical charges.)
1.
A chemical bond formed when two atoms
share electrons
2.
Students should circle the two electrons
between the two “F’s” on the right.
3.
molecule
4.
double bond
5.
True
6.
in molecules
7.
d
8.
Atoms of some elements in a molecular
compound pull more strongly on shared
electrons than do atoms of other elements. As a
result, the electrons are pulled more toward one
atom, causing the bonded atoms to have slight
electrical charges.
9.
polar
10.
equally
11.
If two atoms pull on shared electrons with
equal strength in opposite directions, the polar
bonds cancel each other out.
12.
True
13.
Because polar molecules attract each other
much more than nonpolar molecules do
14.
Oil molecules are nonpolar, so they are not
attracted to the polar water molecules, which
are attracted more strongly to each other than to
the molecules of oil.
15.
Detergent causes the dirt and water to mix,
because detergent molecules have a nonpolar
end that is attracted to oil molecules and a polar
end that is attracted to water molecules
5.4 Bonding in Metals
Guided Reading and Study
Use Target Reading Skills
Graphic organizers should show that metallic
bonding causes the properties of metals,
which include electrical conductivity, heat
conductivity, ductility, malleability, and luster.
Some students may describe ductility and
malleability simply as the ability to change
shape.
1. alloy
2. Ability to conduct heat, ability to conduct
electricity, ability to change shape easily, luster
3. Stainless steel; as strong as iron but will not
react with air and water as iron does; can be
used to make tools
4. a, c, d
5. Positively charged metal ions embedded in
a “sea” of valence electrons
6. Attractions between the positive metal ions
and the “sea” of electrons around them
7. (Accept any correct examples of uses given
for each property.) Conduct heat: Loosely held
electrons can move, transferring thermal
energy; metal frying pan. Conduct electricity:
Current flows because electrons are free to
move; copper wire. Ability to change shape:
Metal ions are attracted by loose electrons all
around them but not to other metal ions; metal
can be bent, hammered or drawn into wire
without breaking; metal sculpture. Luster: Light
strikes valence electrons and is given off again;
mirror.