1. Element vs. Compound Fe Element C Cl2 FeCl2 Compound CCl4 Table 1.
Chemical Formula
Element or Compound? Fe
Element C
Cl2
FeCl2
Compound
CCl4

2. 1. What does the subscript 2 indicate in Cl2?
There are 2 Cl atoms.
2. What is implied if there is no subscript?
There is only 1 atom present.

3. 3. Classify C, Fe, and Cl as metals or nonmetals.
4. True or False: “The formulas for elements never contain a subscript.”
False:
Cl2 is an element, but it has a subscript

4. 6. Why? Element There is only 1 type of atom present.
5. Would you expect the formula S8 to represent a compound or an element?
Element
6. Why?
There is only 1 type of atom present.

5. 7. Classify as element or compound.
CsOH
NaBr
PF5 CO
H2O
HCl
element
CaCl2
Br2
SiO2 P4
KCl O2 Ag
compound
element
compound
compound
compound
element
compound
compound
compound
element
compound
element

6. “It is quality rather than quantity that matters.” – Lucius Annaeus
Honors Chemistry /17/13
“It is quality rather than quantity that matters.” – Lucius Annaeus
DO NOW:
In your notes: What part of the atom contains almost all of the atom’s mass?
AGENDA:
Students will be able to describe the difference between an ionic and covalent compound by reviewing our worksheet.
HOMEWORK:
1. Finish book work from last week for tomorrow.
ANNOUNCEMENT:
1. Science club is meeting today! 

7. In your textbook: read section 7
In your textbook: read section 7.2 (starts on page 210) and answer the following questions: On page 232: numbers 60, 62, 63, 64, 66, 67

8. Multiple capital letters
8. What clues are given in chemical formulas to differentiate between an element and a compound?
Multiple capital letters

9. Notes Subscript number = number of each atom present
No subscript = 1 atom present
Element: made up of only 1 type of atom
may have more than 1 atoms

10. Notes Diatomic Elements Uncle HOFBrINCl H2 O2 F2 Br2 I2 N2 Cl2
2 atoms present
Only certain elements exist as diatomic in nature
Uncle HOFBrINCl
H2 O2 F2 Br2 I2 N2 Cl2

11. Notes Compound: made up of more than 1 type of atom
May have metals or nonmetals or both

12. Ionic or Covalent Bond? Table 2. ZnCl2 CCl4 Na2O P2O5 Fe2O3 N2O4 CuI
Ionic Compound
Covalent Compound
ZnCl2
CCl4
Na2O
P2O5
Fe2O3
N2O4
CuI
NI3

13. 1. The compound ZnCl2 is considered to be _____ compound.
Ionic Compound
2. The compound that contains N and O is a ______ compound.
Covalent Compound
3. Does the classification appear to be based on how many atoms are present?
No.

14. 4. Write the symbols for each element present in Table 2.
Ionic
Covalent
ZnCl2
CCl4
Na2O
P2O5
Fe2O3
N2O4
CuI
NI3 C N O Na P Cl Fe Cu Zn I
Ionic = metal + nonmetal
Covalent = nonmetal + nonmetal

15. 6. Classify as ionic or covalent.
NaBr
OF2
CsF2
SF6
NO2
CrCl3
ionic
CoBr2
BaS
CO2
ionic
covalent
ionic
covalent
ionic
covalent
covalent
ionic

16. Notes
Ionic Compound = a compound with a bond between a metal and a nonmetal
Covalent Molecules = a compound with a bond between 2 or more nonmetals

17. Octet Rule
Atoms tend to gain, lose, or share electrons so that they have 8 electrons in their outershell.

19. 1 lose cation K1+ Potassium has ____ valence electrons.
To achieve the octet rule, it would be easier for potassium to ___________ electrons. (gain/lose)
This would make potassium a _____________. (cation/anion)
This is the symbol for potassium’s ion: _________
lose
cation
K1+

20. 2 lose cation Mg2+ Magnesium has ____ valence e-s.
To achieve the octet rule, it would be easier for magnesium to ___________ electrons. (gain/lose)
This would make magnesium a _____________. (cation/anion)
This is the symbol for magnesium’s ion: _________
lose
cation
Mg2+

21. 3 lose cation B3+ Boron has ____ valence electrons.
To achieve the octet rule, it would be easier for boron to ___________ electrons. (gain/lose)
This would make boron a _____________. (cation/anion)
This is the symbol for boron’s ion: _________
lose
cation
B3+

22. 5 gain anion N3- Nitrogen has ____ valence electrons.
To achieve the octet rule, it would be easier for nitrogen to ___________ electrons. (gain/lose)
This would make nitrogen an _____________. (cation/anion)
This is the symbol for nitrogen’s ion: _________
gain
anion
N3-

23. 6 gain anion O2- Oxygen has ____ valence electrons.
To achieve the octet rule, it would be easier for oxygen to ___________ electrons. (gain/lose)
This would make oxygen an _____________. (cation/anion)
This is the symbol for oxygen’s ion: _________
gain
anion
O2-

24. 7 gain anion Cl1- Chlorine has ____ valence electrons.
To achieve the octet rule, it would be easier for chlorine to ___________ electrons. (gain/lose)
This would make chlorine an _____________. (cation/anion)
This is the symbol for chlorine’s ion: _________
gain
anion
Cl1-

25. 7. Why are noble gases inert?
Reactions are movements of electrons.
Noble gases already have 8 valence electrons.
They don’t need to interact with any other elements.

26. 8. What’s the relationship between the charge of an ion and its location in the periodic table?
Elements in the same group tend to have the same charges for their ions.

27. Where do the electrons go … when an atom loses an electron?
To another ATOM!

28. Where does the electron come from…. when an atom gains an electron?
From another ATOM!

29. A bond formed between 2 ions by the transfer of electrons
Ionic Bonding
A bond formed between 2 ions by the transfer of electrons

30. Usually between a metal and a nonmetal
Ionic Bonding
Usually between a metal and a nonmetal
Metals lose electrons
Nonmetals gain electrons

31. Ionic Bonding

32. Ionic Bonding

33. Ionic Bonding

34. Lewis Dots and Ionic Bonding