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Element vs. Compound Fe Element C Cl2 FeCl2 Compound CCl4 Table 1.

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Presentation on theme: "Element vs. Compound Fe Element C Cl2 FeCl2 Compound CCl4 Table 1."— Presentation transcript:

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.

18

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


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