Chemistry

• EVERY CHLORINE ATOM HAS 17 PROTONS, WITHOUT EXCEPTION, –HOWEVER, NOT EVERY CHLORINE ATOM

HAS 18 NEUTRONS.–ATOMS WITH THE SAME NUMBER OF

PROTONS BUT CONTAIN DIFFERENT NUMBERS OF NEUTRONS ARE CALLED ISOTOPES.

• BECAUSE ISOTOPES OF AN ELEMENT HAVE DIFFERENT NUMBERS OF NEUTRONS THEY HAVE DIFFERENT MASS NUMBERS.

• EVERY CHLORINE ATOM HAS 17 PROTONS, WITHOUT EXCEPTION, –HOWEVER, NOT EVERY CHLORINE ATOM

HAS 18 NEUTRONS.–ATOMS WITH THE SAME NUMBER OF

PROTONS BUT CONTAIN DIFFERENT NUMBERS OF NEUTRONS ARE CALLED ISOTOPES.

• BECAUSE ISOTOPES OF AN ELEMENT HAVE DIFFERENT NUMBERS OF NEUTRONS THEY HAVE DIFFERENT MASS NUMBERS.

ISOTOPESISOTOPES

• ISOTOPES ARE CHEMICALLY ALIKE BECAUSE THEY HAVE IDENTICAL NUMBERS OF PROTONS AND ELECTRONS– IT’S THE ELECTRONS AND PROTONS THAT

ARE RESPONSIBLE FOR CHEMICAL BEHAVIOR

• ISOTOPES ARE CHEMICALLY ALIKE BECAUSE THEY HAVE IDENTICAL NUMBERS OF PROTONS AND ELECTRONS– IT’S THE ELECTRONS AND PROTONS THAT

ARE RESPONSIBLE FOR CHEMICAL BEHAVIOR

proton

neutronneutron

electronelectron

BERYLLIUMISOTOPES

BERYLLIUMISOTOPES

EXAMPLE OF AN ISOTOPE

EXAMPLE OF AN ISOTOPE

ClCl3535

1717 ClCl3737

1717

20 20 NEUTRONSNEUTRONS

ATOMIC MASS

1818 NEUTRONSNEUTRONS

ATOMIC NUMBERATOMIC NUMBER

IONSIONS

• AN ELEMENT’S ATOMS ARE NOT ALWAYS NEUTRAL IN CHARGE.– WHEN AN ATOM LOSES OR GAINS ONE OR MORE OF

ITS ELECTRONS IT BECOMES ION.• AN ION THAT HAS MORE ELECTRONS THAN

PROTONS HAS A NEGATIVE ELECTRICAL CHARGE• AN ION THAT HAS FEWER ELECTRONS THAN

PROTONS HAS A POSITIVE ELECTRICAL CHARGE

• AN ELEMENT’S ATOMS ARE NOT ALWAYS NEUTRAL IN CHARGE.– WHEN AN ATOM LOSES OR GAINS ONE OR MORE OF

ITS ELECTRONS IT BECOMES ION.• AN ION THAT HAS MORE ELECTRONS THAN

PROTONS HAS A NEGATIVE ELECTRICAL CHARGE• AN ION THAT HAS FEWER ELECTRONS THAN

PROTONS HAS A POSITIVE ELECTRICAL CHARGE

NOTE: IT’S THE PROTONS THAT DEFINE THE TYPE OF ATOM IT IS, BUT THE ELECTRONS DEFINE THE ATOM’S CHARGE.

NOTE: IT’S THE PROTONS THAT DEFINE THE TYPE OF ATOM IT IS, BUT THE ELECTRONS DEFINE THE ATOM’S CHARGE.

SOME ATOMS GAIN ELECTRONS

SOME ATOMS GAIN ELECTRONS

O

--

----

--

--

--

--

--

O-2

--

----

--

--

--

--

--

----

ATOM’S IONIC CHARGE = # PROTONS - # ELECTRONS

ATOM’S IONIC CHARGE = # PROTONS - # ELECTRONS

The Nerve Cells

Sodium and potassium ions are used in the transmission of a nerve impulse.

Chemical Reactions Ø     Living things undergo thousands of

chemical reactions

Ø     Chemical equations represent chemical reactions

Ø     CO2 + H20-----goes to-----H2CO3

(carbonic acid) is a sample Chemical Reaction in living things

Ø     Reactants are on the left side of the equation, while products are on the right side  

Activation energy is required to start many reactions

Energy must be added to the reactants for most chemical reactions to occur; called activation energy

Enzymes

• Enzymes are chemical substances in living things that act as catalysts & reduce the amount of activation energy needed

• Organisms contain thousands of different enzymes

• Most enzymes end with –ase (e.g. lipase is the enzyme that acts on lipids)

Physical Properties of Water• All of water’s UNIQUE properties are due to its

POLARITY and HYDROGEN BONDING• POLARITY• H2O is a NEUTRAL molecule (p+ = e-)• Oxygen attracts most of the e- toward its end

and away from the hydrogen• The OXYGEN END acts NEGATIVE, while the

HYDROGEN END acts POSITIVE ----- POLARITY (unequal distribution of charge)

HYDROGEN BONDING

Negative OXYGEN of ONE H2O molecule attracts the Positive HYDROGEN of ANOTHER H2O molecule

Bonding Strengths

True chemical bonds like covalent, ionic, and metallic bonds are the strongest bonds• Covalent bonds are the strongest force of

attraction. They are stronger than ionic and metallic bonds.

• Hydrogen Bonding is a weaker type of bonding because it’s between molecules.

Acids and Bases

• The degree of acidity or alkalinity (basic) is important in organisms

• The force of attraction between molecules is so strong that the oxygen atom of one molecule can actually remove the hydrogen from other water molecules; called Dissociation

• H20-----GOES TO----- H+ + OH- • OH- called hydroxide ion; H+ called hydrogen

ion

• Free H+ ion can react with another water molecule to form H3O+ (hydronium ion)

• Acidity or alkalinity is a measure of the relative amount of H+ and OH- ions dissolved in a solution

• Neutral solutions have an equal number of H+

and OH- ions • Acids have more H3O+ ions than OH- ions; taste

sour; and can be corrosive • Bases contain more OH- ions than H3O+ ions;

taste bitter; & feel slippery

PH Scale

• Compares the relative concentration of H3O+

ions and OH- ions • Scale ranges from 0 to

14; 0-3 is very acidic; 7 is neutral; 11-14 is very basic or alkaline

Buffers

• Control of pH is important to organisms • Enzymes function only within a narrow pH

range; usually neutral • Buffers neutral acids or bases in organisms to

help control pH

Organic Molecules

• Organic Compounds - have carbon bonded to other atoms (mostly Hydrogen) and determine structure/function of living things

• Inorganic Compounds – all others• Organic compounds are made from a carbon

skeleton which can – vary in length, – be branched or unbranched– have double bonds which vary in location– or may be arranged in rings.

Types of Organic Molecules

MACROMOLECULES fall into four major groups • 1. Carbohydrates

2. Lipids3. Proteins4. Nucleic Acids