Get ready for Bell Work 1-24-18

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

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

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.

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

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

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Covalent and Metallic Bonds Brain Pop!

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

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

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.

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

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

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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

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

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

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.

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

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)

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.

Covalent bonds – share electrons Both atoms use the same electrons

Ammonia – NH3 Share electrons to have a full outer level

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)

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.

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?

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.

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.

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 _________________.

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

Covalent Bond Worksheet