1. Fig. 2-00

2. Fig. 2-01 H Rb K Na Li Fr Cs Sr Ca Mg Be Ra Ba Y Sc Ac La Zr Ti Rf Hf Nb V Db Ta Mo Cr Sg W Tc Mn Bh Re Ru Fe Hs Os Rh Co Mt Ir Pd Ni Uun Pt Xe Kr Uuo Rn Ag Cu Uuu Au Cd Zn Uub Hg Ar Ne In Ga Tl Al B Sn Ge Uuq Pb Si C Sb As Bi P N Te Se Uuh Po S O I Br At Cl F He Th Ce Pa Pr U Nd Np Pm Pu Sm Am Eu Lr Lu Cm Gd Bk Tb Cf Dy Es Ho Fm Er Md Tm No Yb 6 C 12

3. Fig. 2-01a Mercury (Hg)

4. Fig. 2-01b Copper (Cu)

5. Fig. 2-01c Lead (Pb)

6. Fig. 2-02 Carbon (C): 18.5% Hydrogen (H): 9.5% Nitrogen (N): 3.3% Calcium (Ca): 1.5% Trace elements: less than 0.01% Boron (B) Manganese (Mn) Oxygen (O): 65.0% Magnesium (Mg): 0.1% Phosphorus (P): 1.0% Potassium (K): 0.4% Sulfur (S): 0.3% Sodium (Na): 0.2% Chlorine (Cl): 0.2% Cobalt (Co) Chromium (Cr) Iron (Fe) Iodine (I) Fluorine (F) Copper (Cu) Silicon (Si) Zinc (Zn) Vanadium (V) Tin (Sn) Molybdenum (Mo) Selenium (Se)

7. Fig. 2-03

8. Fig. 2-03a

9. Fig. 2-03b

10. Fig. 2-04 Nucleus Protons Neutrons Electrons Nucleus Cloud of negative charge (2 electrons) 2 2 2

11. Fig. 2-05 First electron shell (can hold 2 electrons) Outer electron shell (can hold 8 electrons) Hydrogen (H) Atomic number = 1 Carbon (C) Atomic number = 6 Nitrogen (N) Atomic number = 7 Oxygen (O) Atomic number = 8 Electron

12. Fig. 2-06-1 Outer shell has 1 electron Outer shell has 7 electrons The outer electron is stripped from sodium and completes the chlorine atom’s outer shell Na Sodium atom Cl Chlorine atom

13. Fig. 2-06-2 Outer shell has 1 electron Outer shell has 7 electrons The outer electron is stripped from sodium and completes the chlorine atom’s outer shell Na Sodium atom Cl Chlorine atom Complete outer shells The attraction between the ions—an ionic bond—holds them together Na  Sodium ion Cl  Chlorine ion Sodium chloride (NaCl)

14. Fig. 2-07 Name (molecular formula) Hydrogen gas (H 2 ) Oxygen gas (O 2 ) Methane (CH 4 ) Electron configurationStructural formulaSpace-filling modelBall-and-stick model Single bond (a pair of shared electrons) Double bond (two pairs of shared electrons)

15. Fig. 2-08 Hydrogen bond

16. Fig. 2-09

17. Fig. 2-10 Microscopic tubes Cohesion due to hydrogen bonds between water molecules Evaporation from the leaves SEM Flow of water

18. Fig. 2-10a Evaporation from the leaves Flow of water

19. Fig. 2-10b Microscopic tubes Cohesion due to hydrogen bonds between water molecules SEM

20. Fig. 2-11

21. Fig. 2-12

22. Fig. 2-13 Hydrogen bond Liquid water Ice

23. Fig. 2-14 Sodium ion in solution Chloride ion in solution Salt crystal Na  Cl –

24. Fig. 2-15

25. Fig. 2-16 Basic solution Neutral solution Acidic solution Oven cleaner Household bleach Human blood Pure water Grapefruit juice, soft drink Lemon juice, gastric juice Household ammonia Milk of magnesia Seawater Tomato juice Urine pH scale 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Increasingly acidic (greater H  concentration) Increasingly basic (lower H  concentration) Neutral [ H + ]  [ OH – ]

26. Fig. 2-16a Basic solution Neutral solution Acidic solution

27. Fig. 2-17

28. Fig. 2-18

29. Fig. 2-T01

30. Fig. 2-UN01 HH O

31. Fig. 2-UN02 HH O (slightly  ) (slightly –)

32. Fig. 2-UN03 2 H 2 2 H 2 O O2O2 Hydrogen gas Oxygen gas Water ProductsReactants  

33. Fig. 2-UN04

34. Fig. 2-UN05 Proton Positive charge Determines element Neutron No charge Determines isotope Electron Negative charge Participates in chemical reactions Outer-shell electrons determine chemical behavior Nucleus Consists of neutrons and protons Atom

35. Fig. 2-UN06 Attraction between oppositely charged ions holds the ions in an ionic bond. Lithium fluoride (ionic compound) Lithium ionFluoride ion

36. Fig. 2-UN07 Electron sharing Atoms joined into a molecule via covalent bonds

37. Fig. 2-UN08 Hydrogen bond

38. Fig. 2-UN09 Neutral Basic Acidic pH scale 14 7 0 Lower H + concentration H + concentration equal to OH – concentration Greater H + concentration [H+][H+] = [ OH  ]

39. Fig. 2-UN10

40. Fig. 2-UN11 Fluorine atomPotassium atom