Fig. 2-00

Fig 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

Fig. 2-01a Mercury (Hg)

Fig. 2-01b Copper (Cu)

Fig. 2-01c Lead (Pb)

Fig 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)

Fig. 2-03

Fig. 2-03a

Fig. 2-03b

Fig Nucleus Protons Neutrons Electrons Nucleus Cloud of negative charge (2 electrons) 2 2 2

Fig 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

Fig 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

Fig 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)

Fig 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)

Fig Hydrogen bond

Fig. 2-09

Fig Microscopic tubes Cohesion due to hydrogen bonds between water molecules Evaporation from the leaves SEM Flow of water

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

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

Fig. 2-11

Fig. 2-12

Fig Hydrogen bond Liquid water Ice

Fig Sodium ion in solution Chloride ion in solution Salt crystal Na  Cl –

Fig. 2-15

Fig 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 Increasingly acidic (greater H  concentration) Increasingly basic (lower H  concentration) Neutral [ H + ]  [ OH – ]

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

Fig. 2-17

Fig. 2-18

Fig. 2-T01

Fig. 2-UN01 HH O

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

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

Fig. 2-UN04

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

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

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

Fig. 2-UN08 Hydrogen bond

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

Fig. 2-UN10

Fig. 2-UN11 Fluorine atomPotassium atom