1. Get ready for Bell Work

2. 1. Which option contains only compounds?
A. H2O, H2O2, H3O, CO2
B. Na, NaCl, Pb, C6H12O6
C. NH3, KNO3, Hg, Ne
D. Au, Ni, Cu, Fe

3. 2. Which of these is a compound? a. H2O b. Co c. Mn d. S

4. 3. Lisa was thirsty and decided to prepare some Kool-aid
3. Lisa was thirsty and decided to prepare some Kool-aid. She combined Kool-aid powder, water, and sugar in a glass pitcher.
Which of the following statements best describes how she can know if this drink is a mixture or compound?
It is a mixture because she can separate all of the individual ingredients
b. It is a compound because it tastes different after you add in the sugar.
c. It’s a mixture because a reaction occurred when the ingredients were combined.

5. 4. Which of the following best describes an atom. a
4. Which of the following best describes an atom? a. protons and electrons grouped together in a random pattern b. protons and electrons grouped together in a alternating pattern c. a core of protons and neutrons surrounded by electrons d. a core of electrons and neutrons surrounded by protons

6. 5.
Which element from Period 2 has the lowest atomic mass? a. Li b. Ca c. Ne

7. 6.

8. 7.

9. Covalent and Metallic Bonds
Brain Pop!

10. 1. Which option contains only compounds?
A. H2O, H2O2, H3O, CO2
B. Na, NaCl, Pb, C6H12O6
C. NH3, KNO3, Hg, Ne
D. Au, Ni, Cu, Fe

11. 2. Which of these is a compound? a. H2O b. Co c. Mn d. S

12. 3. Lisa was thirsty and decided to prepare some Kool-aid
3. Lisa was thirsty and decided to prepare some Kool-aid. She combined Kool-aid powder, water, and sugar in a glass pitcher.
Which of the following statements best describes how she can know if this drink is a mixture or compound?
It is a mixture because she can separate all of the individual ingredients
b. It is a compound because it tastes different after you add in the sugar.
c. It’s a mixture because a reaction occurred when the ingredients were combined.

13. 4. Which of the following best describes an atom. a
4. Which of the following best describes an atom? a. protons and electrons grouped together in a random pattern b. protons and electrons grouped together in a alternating pattern c. a core of protons and neutrons surrounded by electrons d. a core of electrons and neutrons surrounded by protons

14. 5.
Which element from Period 2 has the lowest atomic mass? a. Li b. Ca c. Ne

15. 6.

16. 7.

17. Success Criteria:
1. I can determine Valence Electrons by looking at the Periodic Table. They are used for BONDING
2. I can differentiate between Covalent and Metallic Bonding.
TOC:
#8. Covalent and Metallic Bond Notes
#9. Covalent Bond Worksheet

18. Ionic Bonding Worksheet
Elbow Partners: Fill in the chart below Cl K Mg F 17 Al Na N O C

19. Covalent and Metallic Bonds
Explain how covalent bonds form.
Explain how metallic
bonds form.

20. Covalent and Metallic bonds
Covalent bonds usually form between atoms of nonmetals.
A covalent bond forms when atoms share one or more pairs of electrons.

21. Substances containing covalent bonds consist of individual particles called molecules.
Most molecules are
composed of atoms
of two or more
elements.

22. Covalent compounds and molecules
A molecule is the smallest particle into which a covalently bonded compound can be divided and still be the same compound.
(H2O is still water even if there is just one molecule of it)

23. One way to represent atoms and molecules is to use electron-dot diagrams. An electron-dot diagram shows only the valence electrons in an atom.

24. Covalent bonds – share electrons
Both atoms use
the same electrons

25. Ammonia – NH3 Share electrons to have a full outer level

26. Properties of covalent bonds
Substances that have covalent bonds tend to have:
Low melting point
Low boiling point
Are brittle in the solid state
(examples: oxygen has a low boiling point, wood is brittle and breaks when bent)

27. A metallic bond is formed by the attraction between positively charged metal ions and the electrons in the metal.
Bonding in metals is a result of the metal atoms being so close to one another that their valence levels overlap. This overlapping allows valence electrons to move throughout the metal.

28. Properties of metallic bonds
Metallic bonding gives metals their particular properties:
Electrical conductivity
Malleability
Ductility
Review with your table group what these three properties are; and if they are physical or chemical properties?

29. Electrical Conductivity
Metallic bonds allow metals to conduct electrical current. When you turn on a lamp, electrons move within the copper wire that connects the lamp to the outlet. The electrons that move are the valence electrons.
These electrons are free to move because the electrons are not connected to
any one atom.

30. Ductility and Malleability
Ductility is the ability to be drawn into
wires.
Example – copper can be made into wires for electrical cords.
Malleability is the ability to be hammered into sheets.
Example – is aluminum can be pounded into thin sheets.
Moving electrons maintain the metallic bonds no matter how the shape of the metal changes. Which means metal objects can be bent without being broken.

31. What is a covalent bond?
Atoms ___________ one or more electrons with each other to form the bond.
Each atom is left with a ________________ outer shell.
A covalent bond forms between two _________________.

32. What is a covalent bond?
Atoms ___________ one or more electrons with each other to form the bond.
Each atom is left with a ________________ outer shell.
A covalent bond forms between two _________________.
SHARE
COMPLETE
NONMETAL

33. Covalent Bond Worksheet