INORGANIC CHEMISTRY EVERYTHING IS MADE OF ELEMENTS

ELEMENTS 92 NATURALLY OCCURRING HYDROGEN LIGHTEST URANIUM HEAVIEST

BIG SIX ELEMENTS OXYGEN CARBON HYDROGEN NITROGEN CALCIUM PHOSPHORUS

ATOMS SMALLEST PARTICLES OF ELEMENTS PROTONS –UNCHARGED PARTICLES ELECTRONS –NEGATIVELY CHARGED PARTICLES NEUTRONS –POSITIVELY CHARGED PARTICLES

Protons and neutrons are in the nucleus. Electrons move around the nucleus. The Study of Atoms Figure 2.1

ATOMIC NUMBER NUMBER OF PROTONS IN NUCLEUS

ATOMIC MASS PROTONS + NEUTRONS EQUAL MASS

ISOTOPES OF AN ELEMENT ARE ATOMS WITH DIFFERENT NUMBERS OF NEUTRONS. ISOTOPES OF OXYGEN ARE: EACH CHEMICAL ELEMENT HAS A DIFFERENT NUMBER OF PROTONS. ISOTOPES

ELECTRONS ARE ARRANGED IN ELECTRON SHELLS CORRESPONDING TO DIFFERENT ENERGY LEVELS

OCTET RULE ATOMS ARE MOST STABLE WHEN THEIR OUTERMOST SHELLS ARE FILLED WITH 2 ELECTRONS THE FIRST FEW ELEMENTS & 8 ELECTRONS FOR THE LARGER ATOMS

CHEMICAL COMPOUNDS

CHEMICAL FORMULAS DESCRIBE COMPOSITION AND STRUCTURE OF ELEMENTS AND COMPOUNDS

STRUCTURAL ISOMERS SAME CHEMICAL FORMULA DIFFERENT ARRANGEMENTS

CHEMICAL EQUATIONS REACTANTS ON THE LEFT PRODUCTS ON THE RIGHT

NOBLE GASES INERT ATOMS TEND TO LOSE OR GAIN ELECTRONS TO FILL THEIR OUTER SHELLS

ATOMS FORM MOLECULES ATOMS COMBINE TO COMPLETE THE OUTERMOST SHELL THE NUMBER OF MISSING OR EXTRA ELECTRONS IN THIS SHELL IS THE VALENCE COMBINE IN FIXED RATIOS

A compound contains different kinds of atoms. The forces holding atoms in a compound are chemical bonds. How Atoms Form Molecules: Chemical Bonds

CHEMICAL BONDS IONIC COVALENT

The number of protons and electrons is equal in an atom. Ions are atoms that have gained or lost electrons and are charged. How Atoms Form Molecules: Chemical Bonds Figure 2.2a

Covalent bonds form when two atoms share one or more pairs of electrons. Covalent Bonds Figure 2.3a

POLAR COVALENT BONDS

Hydrogen bonds form when a hydrogen atom covalently bonded to an O or N atom in another molecule. Hydrogen Bonds Figure 2.4

Ionic bonds are attractions between ions of opposite charge. One atom loses electrons and another gains electrons. Ionic Bonds Figure 2.2b

CHEMICAL REACTIONS INVOLVE THE MAKING OR BREAKING OF BONDS BETWEEN ATOMS. A CHANGE IN CHEMICAL ENERGY OCCURS DURING A CHEMICAL REACTION. ENDERGONIC REACTIONS ABSORB ENERGY. EXERGONIC REACTIONS RELEASE ENERGY. CHEMICAL REACTIONS

METABOLIC CHEMICAL REACTIONS ARE REVERSIBLE USUALLY LITTLE FREE DIFFERENCE BETWEEN REACTANTS AND PRODUCTS THIS MEANS AS LONG AS EXTERNAL ENERGY IS AVAILABLE MOST REACTINS IN LIVING CELLS ARE THEORETICALLY REVERSIBLE –ALLOWS CELLS TO CONTROL RELEASE OF FREE ENERGY –ALLOWS CELLS TO RESYNTHESIZE BIOLOGICAL MOLECULES

THE DIRECTION OF A REVERSIBLE REACTION WILL DEPEND ON: – THE CONCENTRATIONS OF THE CHEMICALS –THEIR ENERGY RELATIONSHIPS –THEIR SOLUBILITY

TYPES OF CHEMICAL REACTIONS SYNTHESIS REACTIONS DECOMPOSITION REACTIONS EXCHANGE REACTIONS REVERSIBLE REACTIONS

Occur when atoms, ions, or molecules combine to form new, larger molecules Anabolism is the synthesis of molecules in a cell. Synthesis Reactions

Occur when a molecule is split into smaller molecules, ions, or atoms. Catabolism is the decomposition reactions in a cell. Decomposition Reactions

Are part synthesis and part decomposition. Exchange Reactions

Can readily go in either direction. Each direction may need special conditions. Reversible Reactions

REDOX REACTIONS REDOX REACTIONS: PAIRED OXIDATION AND REDUCTION REACTIONS OXIDATION: LOSS OF ELECTRONS REDUCTION: GAIN IN ELECTRONS ORGANIC MOLECULES LOSE HYDROGEN ATOMS RATHER THAN JUST ELECTRONS

METABOLISM ALL THE REACTIONS THAT OCCUR IN THE CELL

WATER THE REASON WHY LIFE CAN SURVIVE HERE ON EARTH

PROPERTIES OF WATER POLAR MOLECULE EXCELLENT SOLVENT COHESIVE ADHESIVE TENDS TO MAINTAIN A STABLE TEMPERATURE HIGH SPECIFIC HEAT

WATER IS A POLAR MOLECULE

EACH WATER MOLECULE FORM FOR A MAXIMUM OF FOUR HYDROGEN BONDS

Solvent –Polar substances dissociate, forming solutes WATER AS A SOLVENT

WATER AND CAPILLARY ACTION ADHESIVE AND COHESIVE QUALITIES

Hydrogen bonding between water molecules makes water a temperature buffer. WATER AS A TEMPERATURE BUFFER Figure 2.4b

HEAT OF VAPORIZATION IT TAKE 540 CALORIES TO CHANGE ONE GRAM OF LIQUID WATER INTO ONE GRAM OF WATER VAPOR

HEAT OF FUSION WATER LOSES 80 CALORIES PER GRAM AS IT TURNS TO ICE

WATER BECOMES LESS DENSE AS IT FREEZES REACHES MAXIMUM DENSITY AT 4 DEGREES C EXPANDS AGAIN AS TEMPERATURE EXPANDS THIS IS WHY LAKES AND POOLS FREEZE FROM SURFACE DOWN & ICE FLOATS

ALL CHEMICAL REACTIONS IN THE CELLS AND EXTRACELLULAR FLUIDS TAKE PLACE IN SOLUTION H + AND OH  PARTICIPATE IN CHEMICAL REACTIONS Water

An acid is a substance that dissociates into one or more H +. HCl  H + + Cl  ACIDS Figure 2.6a

A base is a substance that dissociates into one or more OH . NaOH  Na + + OH  BASES Figure 2.6b

A salt is a substance that dissociates into cations and anions, neither of which is H + or OH . NaCl  Na + + Cl  SALTS Figure 2.6c

DISSOLUTION OF SALTS

IMPORTANCE OF SALTS SOURCE OF MINERAL IONS ESSENTIAL FOR: –FLUID BALANCE –ACID-BASE BALANCE –NERVE AND MUSCLE FUNCTION –BLOOD CLOTTING –BONE FORMATION –ETC

The amount of H + in a solution is expressed as pH. pH =  log[H + ] Increasing [H + ], increases acidity. Increasing [OH  ] increases alkalinity. Most organisms grow best between pH 6.5 and 8.5. Acid-Base Balance

BUFFERS OPERATE TO MAINTAIN APPROPRIATE pH levels WEAK ACID, WEAK BASE AND THE SALT OF THE ACID AND BASE

SODIUM BICARBONATE- CARBONIC ACID BUFFER SYSTEM COMMON BUFFERING SYSTEM

Figure 2.7