1. Bonding Review Standard 2

2. Standard 2a. 1.0 What is the difference between an atom and a molecule? An atom is the smallest, complete part of an element. An atom has no charge. An atom is the smallest, complete part of an element. An atom has no charge. A molecule is when 2 or more atoms combine to form compound. A molecule is the smallest, complete part of a compound. A molecule is when 2 or more atoms combine to form compound. A molecule is the smallest, complete part of a compound.

3. 2. How do molecules behave in: a. Ionic bond: Electrons are transferred, exchanged, or given up/taken b. Covalent bond Electrons are shared c. Metallic bond Electrons are adopted by several different metals

4. 3. Name at least 2 characteristics for: Ionic bond: Ionic bond: Electrostatic lattice, high melting point, high boiling point, crystal, hard brittle, salts Covalent bond: Covalent bond: Low melting point, low boiling point, soft, gases at room temperature Metallic bond: Metallic bond: Electron sea model, delocalized electrons, high melting point, high boiling point, malleable, ductile, good conductors

5. 4. What is a positive ion called? Anion Anion 5. What is a negative ion called? Ca + ion Ca + ion

6. 6. What are three properties of metallic bonds? Malleable: because the electrons are not associated with any particular nucleus, they can move as they wish. When you hit a metal, the electrons just move. Malleable: because the electrons are not associated with any particular nucleus, they can move as they wish. When you hit a metal, the electrons just move. Ductile: because the electrons are not associated with any particular nucleus, they can move as they wish. When you shape a metal into thin strings of wire, the electrons just line up in single file lines. Ductile: because the electrons are not associated with any particular nucleus, they can move as they wish. When you shape a metal into thin strings of wire, the electrons just line up in single file lines. Good Conductors: Because electrons can move pretty freely, they are able to carry and distribute heat and electricity. Good Conductors: Because electrons can move pretty freely, they are able to carry and distribute heat and electricity.

7. 7. In a formula, what does a subscript represent? It represents how many of each atom is present. It represents how many of each atom is present. For H 2 O, there are 2 hydrogens and 1 oxygen. For H 2 O, there are 2 hydrogens and 1 oxygen. For Al 2 S 3, there are 2 aluminum and 3 sulfur. For Al 2 S 3, there are 2 aluminum and 3 sulfur.

8. 8. What is the difference between a polyatomic and a monoatomic ion? Monoatomic Ion: A charged particle made from 1 atom Monoatomic Ion: A charged particle made from 1 atom F- F- Polyatomic Ion: A charged particle made from 2 or more atoms that are grouped together Polyatomic Ion: A charged particle made from 2 or more atoms that are grouped together CO 3 2- CO 3 2-

9. 9. What are the 6 polyatomic ions you must memorize? Name FormulaCharge Name FormulaCharge Carbonate CO 3 -2 Hydroxide OH-1 Nitrate NO 3 -1 Permanganate MnO 4 -1 Ammonium NH 4 +1 Phosphate PO 4 -3

10. 10. Why do atoms transfer or share electrons? To achieve an octet of electrons like the really cool Noble Gases. To achieve an octet of electrons like the really cool Noble Gases. The only exception is Helium!! It has 2 electrons. The only exception is Helium!! It has 2 electrons.

11. Standard 2b. 1. Using the periodic table, how do you know if a compound is ionic or covalent? If the first element is on the LEFT side of the periodic table, in groups 1-3 it is IONIC If the first element is on the LEFT side of the periodic table, in groups 1-3 it is IONIC If the first element is on the RIGHT side of the periodic table, in groups 4-7 it is COVALENT If the first element is on the RIGHT side of the periodic table, in groups 4-7 it is COVALENT

12. 2. In the compound N 2 P 5, how many Nitrogen are there? There are 2. There are 2. 3. What is a diatomic molecule? It is a covalent molecule where 1 or the 7 diatomic gases are bonded to itself. It is a covalent molecule where 1 or the 7 diatomic gases are bonded to itself. N 2, O 2, F 2, Cl 2, Br 2, I 2, H 2 N 2, O 2, F 2, Cl 2, Br 2, I 2, H 2

13. 4. Name the following compounds a. H 2 Hydrogen gas b. CH 4 Carbon tetrahydride c. NH 3 Nitrogen trihydride d. N 2 nitrogen gas e. Cl 2 chlorine gas

14. Standard 2c 1. What does electrostatic mean? It is a key word for ionic bonds. It is a key word for ionic bonds. It means that positive and negative charges are interlaced between each other. It means that positive and negative charges are interlaced between each other.

15. 2. What type of bond holds NaCl together? Na is on the LEFT so it is IONIC Na is on the LEFT so it is IONIC 3. Draw a picture to show that NaCl is a repeating pattern of positive and negative ions.

16. Standard 2e 1. Draw the Lewis Dot structures for: a. Na b. F c. Mg d. Ne Na F Mg Ne

17. Standard 2g 1. Elements with high electronegativity like Fluorine, will do what to form an ionic bond? Take valence electron from a metal. Take valence electron from a metal. 2. Elements with low ionization energy like Francium, will do what to form an ionic bond? Give up valence electrons to a non metal. Give up valence electrons to a non metal.

18. 3. What happens when 2 elements with high electronegativity try to form a bond? Neither non metal wants to give up an electron, so Neither non metal wants to give up an electron, so They will share the valence electrons and form a COVALENT bond They will share the valence electrons and form a COVALENT bond

19. Neither wants to take any valence electrons, so Neither wants to take any valence electrons, so They form partnership where they look out for each other’s electrons and form a METALLIC bond They form partnership where they look out for each other’s electrons and form a METALLIC bond 4. What happens when 2 elements with low ionization energy try to form a bond?

20. General Test Prep: TiCl 3 Ionic Ionic Transition metal, needs roman numerals Transition metal, needs roman numerals Titanium (III) chloride Titanium (III) chloride

21. Hydrogen Iodide Ionic Ionic No transition metal, so no roman numerals needed No transition metal, so no roman numerals needed HI HI

22. CO 2 Covalent Covalent Carbon dioxide Carbon dioxide

23. Chromium (II) nitrate Ionic Ionic Transition metal, so I need roman numerals Transition metal, so I need roman numerals Polyatomic from pg 224 Polyatomic from pg 224 +3 Cr NO 3 -1 +3 Cr NO 3 -1 Cheerleading maneuver Cheerleading maneuver Cr (NO 3 ) 3 Cr (NO 3 ) 3

24. CaCl 2 Ionic Ionic Not a transition metal, so no roman numerals needed Not a transition metal, so no roman numerals needed Calcium chloride Calcium chloride

25. Rubidium hydroxide Ionic Ionic No transition metal, so no roman numerals needed No transition metal, so no roman numerals needed Polyatomic from pg 224 Polyatomic from pg 224 +1 Rb OH -1 +1 Rb OH -1 RbOH RbOH

26. Na 2 CO 3 Ionic Ionic Not a transition metal, so no roman numerals needed Not a transition metal, so no roman numerals needed Polyatomic from pg 224 Polyatomic from pg 224 Sodium carbonate Sodium carbonate

27. Carbon tetrachloride Covalent Covalent CCl 4 CCl 4

28. NH 4 NO 3 Ionic ** ammonium is the only polyatomic that is first!! Ionic ** ammonium is the only polyatomic that is first!! Not a transition metal, so no roman numerals needed Not a transition metal, so no roman numerals needed Polyatomics from pg 224 Polyatomics from pg 224 Ammonium nitrate Ammonium nitrate

29. Cu Metallic Metallic copper copper

30. Oxygen gas Covalent Covalent Diatomic molecule Diatomic molecule O 2 O 2

31. 1. What type of bond is formed between calcium and sulfide? a. Covalent b. Ionic c. Metallic d. Van der waals

32. 2. When atoms combine to form a molecule by exchanging electrons, what types of bonds are formed? a. Covalent b. Ionic c. Metallic d. Van der waals

33. 3. Which formula represents sodium carbonate? a. Na 2 CO 3 b. Na 2 CO 4 c. NaCO 3 d. Na 2 CO 2

34. 4. Which formula is correctly paired with its’ name? a. CuO copper (III) oxide b. NiCl 2 nickel (II) chloride c. MgCl 2 magnesium chlorine d. Na 2 Osodium dioxide

35. 5. Which is the best way to express the relationship between hydrogen and fluorine when they combine?

36. 6. Which of the following is formed by an ionic bond? a. Chlorine gas b. glucose (C 6 H 12 O 6 ) c. CO 2 d. salts like NaCl

37. 7. The bonds found in Si2H4 are a. Covalent b. Ionic c. Metallic d. Van der waals

38. 8. Which is a covalent compound? a. GeBr 3 b. NO c. CsCl d. TiF

39. 9. Which of the following are formed by transferring electrons? a. GeBr 3 b. NO c. CCl 4 d. SO 3

40. 10. When atoms of Lithium combine with Chlroine, the Li+ ion are smaller than the Li atom, while the Cl- is larger than the Cl atom. Why? a. The Li and Cl atoms both lost electrons. b. The Li atom lost an electron while the Cl atom gained an electron. c. The Li and Cl atoms both gained electrons. d. The Li atom gained an electron while the Cl atom lost an electron.