Section 2.1

1. Atom:

the smallest unit of matter. Atoms consist of protons, neutrons, and electrons.

2. Element:

One type of atom. It CAN NOT be broken down into a simpler substance. It is a group of atoms of the same type. What makes one element different from another element? It’s # of proton’s!

3. Compound:

Is a substance made of atoms of different elements bonded together in a certain ratio. Example: H20

Atomic Model

Proton: a very small particle of

matter that is part of the nucleus of an

atom and that has a positive

electrical charge

Neutron: a very small particle of

matter that has no electrical charge

and is part of the nucleus of all atoms except hydrogen atoms

Electron: a very small particle of matter that has a negative charge of electricity and that travels around the nucleus of an atom

Isotopes: atoms of the same element with different # of neutrons.

Your # of protons & electrons in an atom are equal

6 C12

6 C13

Bohr’s Atomic Model

Page 35 in textbook

First Shell holds 2 Electrons

Second Shell holds 8 Electrons

Third Shell holds 8 Electrons

Fourth Shell holds 18 Electrons

Fifth Shell holds 18 electrons

Six Shell holds 32 Electrons

10

Ne 20

# of total electrons

Scientist Bohr: depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus

View Atomic Model

With a partner (using a laptop)

Create atoms for 10 elements

When creating atoms:

1.Look at the atomic # - that will tell you how many protons you have

2.Look at the atomic mass, Subtract the Atomic # from the Atomic Mass and that will tell you how many neutrons you have!

3.You have the same # of electrons as protons. You just need to correctly fill each shell! If you forget how many electrons are in each shell, reference your periodic table!

17

ClChlorine 35.45

Atomic #Equals # of protons

Atomic Mass: Equals # of protons plus number of neutrons

4. Ion: Is an atom that has gained or lost one or more electrons in it’s outer valence shell.

5. Ionic Bond: A bond where you lose or gain an electron.

(Ionic Bond View with Covalent Bond animation)

6. Covalent Bond: A bond where atoms share a pair of electrons

Covalent Bond

Covalent Bond

7. Molecule: Two or more atoms held together by covalent bonds.

Example: Co2 Carbon and Oxygen SHARE the electrons in the outer shell.

Section 2.1

NANA

11Na22

ClCl

17Cl

Mass of Na is 22g, loses a electron so now more positive.

Cl gains an electron so becomes more negative!

**Remember electrons have a negative charge**

# of electrons

Section 2.1

Take out your Periodic table: Label

Take out your Periodic table:

Complete the following Chemistry Worksheet

First, write the COMPOUND product you would receive when combining the two elements.

Second, draw the Lewis dot representation of the ionic bonding that is occurring.

** Remember Ionic bonding means you gain or lose an electron.**

Example:

One Carbon plus one Hydrogen equalsCarbon- 4 e outer shell, and 2 in inner shell

C-4 H+1 = CH4 C C

6C

1H

H

H

H

H

HH

H

HEvery bond/line equals

2 electrons

Section 2.1

Organic ChemistryAll about the Element Carbon

Carbon atoms have four electrons in their outer shells, and all four are available for bonding. Carbon can share these electrons in single bonds with up to four other atoms to form very stable structures.

CCarbon can form multiple bonds with up to two other atoms by sharing two or more electrons with another atom; forming double bonds or even triple bonds!

1 line equals 2 electrons

Carbons ability to form four bonds in a single plane makes it uniquely suited to form macromolecules.

Section 2.3

Carbon can also readily form bonds with other carbon atoms to form long, complex molecules. When chemists refer to organic molecules, they generally use structural

formulas. A diagram of the molecule is often more helpful than the name. Because of the high percentage of carbon

and hydrogen in organic molecules, the molecules are drawn without labeling them. Carbon atoms are located where lines intersect, unless otherwise noted, and the 4

bonds around each carbon are understood to be completed by the appropriate number of hydrogens.

Below are examples of some common carbon-containing compounds.

Biological MoleculesBiological molecules are composed of small repeating subunits that bond together to form larger units. The subunits, or building blocks, are called monomers.

Polymers are the complex molecules formed from the repeating subunits.

There are four basic classes of complex organic molecules, or macromolecules, that compose cells:

carbohydrates, proteins, lipids, and nucleic acids

Section 2.3

CarbohydratesCarbohydrates are organic macromolecules that are made up of carbon, hydrogen, and oxygen atoms. These atoms

are combined in a ratio of:1 carbon atom : 2 hydrogen atoms : 1 oxygen atom

The presence of multiple carbon-hydrogen bonds within carbohydrates makes them an excellent source of energy

Carbohydrates may be simple or complex.

The building blocks of carbohydrates are the simple sugars known as monosaccharides. Sugars such as glucose,

fructose, and ribose are all examples of monosaccharides.Monosaccharides can be combined to form more complex

carbohydrates known as polysaccharides. Glycogen, starch, and cellulose are all examples of polysaccharides.

GlucoseStarch

Section 2.3

LipidsLipids are organic macromolecules that are insoluble in

water. This is why lipids are often found in biological membranes and other waterproof coverings (e.g. plasma membrane, intracellular membranes of organelles). These lipids play a vital role in regulating which substances can or

cannot enter the cell.The most important lipids, however, are fats. Triglycerides are a type of fat that contain one glycerol molecule and

three fatty acids.

Section 2.3

LipidsFatty acids are long chains of CH2 units joined together. The fatty acids in saturated fats do not contain any double bonds between the CH2 units whereas the fatty acids in unsaturated fats contain some carbon-carbon double bonds. Saturated fats are found in butter, cheese, chocolate, beef, and coconut oil. Unsaturated fats are found in olives and olive oil, peanuts and peanut oil, fish, and mayonnaise. Fats are important because they are a major source of energy. Since they contain even more carbon-hydrogen bonds than carbohydrates, fatty tissue has the ability to store energy for extended periods of time

Unsaturated means containing a carbon double or triple bond.

Section 2.3

ProteinsProteins are organic macromolecules that are composed of amino acid monomers. There are 20 essential amino acids that are used by all living things to construct proteins. These amino acids are made up of the elements carbon, hydrogen, oxygen, and nitrogen. Some of the amino acids also contain sulfur. Three of the amino acids are shown below.

Proteins differ from each other due to the number and arrangement of their component amino acids. Proteins also take on unique shapes as determined by their amino acid sequences.

Proteins are different then Carbohydrates because they can catalyze biochemical reactions. (Enzymes are proteins)

There are three main components of an amino acid, shown to the left.

Section 2.3

Carbohydrates vs. Proteins

• Proteins are made up of the elements C,H,O, and N while Carbohydrates only contain C,H, and O (elemental ratio of these three is 1:2:1)

Protein

Carbohydrate

Section 2.3

Carbohydrates vs. ProteinsFunctions

• Carbohydrates are our essential energy molecules to be use almost immediately (simple sugars like glucose) or stored in the liver as glycogen.

• Proteins are building and regulatory compounds (such as hormones and enzymes). Muscles and cell membranes contain proteins

(why weight lifters eat a lot of protein)

Nucleic AcidsNucleic acids are formed from nucleotide monomers. Nucleotides are chemical compounds that are primarily comprised of the elements carbon, hydrogen, oxygen, nitrogen, and phosphorus. They consist of a five-carbon sugar, a nitrogenous base, and one or more phosphate groups.There are two main types of nucleic acids - ribonucleic acids (RNA) and deoxyribonucleic acids (DNA). These nucleic acids are different because their five-carbon sugars are different. RNA contains ribose, and DNA contains deoxyribose.

There are five nitrogenous bases found in nucleic acids. Adenine (A), cytosine (C), and guanine (G) are found in both DNA and RNA. Thymine (T) is only found in DNA, and uracil (U) is only found in RNA.

Section 2.3

Section 2.3

1. Monomer: molecular subunit of a polymer

2. Polymer: large carbon based molecule formed by monomers.

3. Carbohydrate: molecule composed of carbon, hydrogen, and oxygen; including sugars and starches.

4. Lipid: nonpolar molecular composed of carbon, hydrogen, and oxygen; includes fats and oils.

Section 2.3

1. Fatty Acid: hydrocarbon chain often bonded to glycerol in a lipid.

A triglyceride is three fatty acids and a glycerol.The red portion of the diagram is one glycerol.  Each black chain is a  fatty acid.

1.Protein: polymer composed of amino acids linked to peptide bonds, Any of a group of complex organic macromolecules that contain carbon, hydrogen, oxygen, nitrogen, and usually sulfur and are composed of one or more chains of amino acids

2.Amino Acid: Molecule that makes up proteins; composed of carbon, hydrogen, oxygen, nitrogen, and sometimes sulfur, building blocks of proteins.

3.Nucleic Acid: polymer of nucleotides; the genetic material of organisms, carries genetic information directing all cellular functions DNA.

Dalton’s Atomic Theory

The main points of Dalton's atomic theory were:

•Elements are made of extremely small particles called atoms.•Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties.•Atoms cannot be subdivided, created, or destroyed.•Atoms of different elements combine in simple whole-number ratios to form chemical compounds.•In chemical reactions, atoms are combined, separated, or rearranged.

Dalton’s Atomic TheoryLaw of Conservation of Mass: No detectable gain or loss of mass occurs in chemical reactions. Mass is conserved.

This is why all chemical reactions are balanced on both sides

Example: 2C4H10 + 13O2 8CO2 + 10H2O

C= 8 C=8

H=10 H=10

O=26 O=26

Law of Definite Proportions: In a given chemical compound, the elements are always combined in the same proportions by mass.

Example: H2O always 2 H’s to every 1 O

How many atoms of each element are in the formulas?

C-4 H+1 = CH4

1.Al2 (SO4)3

Al=2 S= 3 O=12

2. CoCl3 ·6H2O

Co= 1 H=12

Chemical Equation

Zn + S ZnS

ReactantsProduct

** No gain or loss of mass occurs in chemical reactions**

** Manipulate Coefficients to make an equation conform to the law of conservation of mass**

Example: Mg (OH)2 + 2HCL MgCL2 __H2O

Mg=1 H=4 Mg=1 H=2 O=1

Cl=2 Cl=2 Need 2 H and a O

O=2

2

Section 2.2 Periodic Table

1. Hydrogen Bond:

a weak chemical bond between an electronegative atom, such as fluorine, oxygen, or nitrogen, and a hydrogen atom bound to another electronegative atom.

2. Cohesion:

is the property of like molecules (of the same substance) to stick to each other due to mutual attraction. Ex: H2O molecules sticking together

3. Adhesion:

is the property of different molecules or surfaces to cling to each other. Example: H2O in a tube creating a meniscus

4.Solution:

A homogeneous mixture of two or more substances

Section 2.2

1. Solvent:

the liquid in which a solute is dissolved to form a solution.

2. Solute:

the substance dissolved in a given solution

3. Acid:

Substance that donates hydrogen ions. Has a pH of less than 7.

4. Base: A substance that accepts hydrogen ions, has a ph between 7 and 14.

5. PH: How Acidity and alkalinity are measured.

Section 2.4

1. Chemical Reaction: a process that involves changes in the structure and energy content of atoms, molecules, or ions.

2. Reactant: The substance that is present at the start of the reaction. Also is the substance that is changed during the chemical reaction.

3. Product: A substance resulting from a chemical reaction.

4. Bond Energy: measure of strength in a chemical bond. The amount of energy it will take to break a bond between two atoms.

Section 2.4

1. Equilibrium: when both the reactants and products are made at the same rate.

2. Activation Energy: Is the amount of energy that needs to be absorbed for a chemical reaction to start.

Page 51 in textbook

1.Exothermic: Chemical reaction releases more energy than it absorbs. If the products have a lower bond energy than the reactants, the reaction is exothermic.

2.Endothermic: Chemical Reaction absorbs more energy than it releases. If products have a higher bond energy than reactants, the reaction is endothermic.

When trying to classify a process as exothermic or endothermic, watch how the temperature of the surroundings changes. An exothermic process releases heat, and causes the temperature of the immediate surroundings to rise. An endothermic process absorbs heat and cools the surroundings.

Examples: Exothermic- Making ice cubes Endothermic-melting ice cubes

Releases energy!

Add H2O reaction occursEnergy is transferred through heat and light

Section 2.5

1. Catalyst:

substance that causes or accelerates a chemical reaction without itself being affected.

2. Enzyme:

a substance produced by a living organism that acts as catalyst to bring about a specific biochemical reaction.

3. Substrate:

Is the material on which an enzyme acts on. It is the reactant that binds to the catalyst.

_______________________ALL MADE OF ATOMS

________________

________________

•The smallest basic unit of _______________

•Consist of three types of smaller particles:

•_________________- _______________________

•_________________- _______________________

•_________________- ________________________

MATTER

PROTONS

NEUTRONS

ELECTRONS

Positive Charge

No Charge

Negative Charge

PROTONS

NEUTRONS

_________________ELECTRONS

•One type of _______________

•Cannot be _________ _______ into a simpler substance.

•Examples:

Gases Metals

________________ ________________

________________ ________________

ATOM

BROKEN DOWN

HYDROGEN

OXYGEN

ALUMINUM

GOLD

What makes one element different from another?

________________________The number of PROTONS

•A SUBSTANCE MADE OF ATOMS(OR ______________) THAT ARE _____________ TOGETHER IN A CERTAIN RATIO.

•EXAMPLES

________________ _______________________

ELEMENTSBONDED

WATER ( H2O ) CARBON DIOXIDE ( CO2 )

• AN ATOM THAT HAS ___________ OR ___________ ONE OR MORE ELECTRONS.

•ATOMS BECOME IONS WHEN THEIR ______________________________________________

•POSITIVELY CHARGED IONS – ________ ELECTRONS

•NEGATIVELY CHARGED IONS – _______ ELECTRONS

•IONS FORM BECAUSE ATOMS ARE MORE STABLE WHEN THEIR _____________ ENERGY LEVEL IS _______.

•________________________ IONS ARE ATTRACTED TO _________________________ IONS

GAINED LOST

NUMBER OF ELECTRONS IS CHANGED

LOSE

GAIN

OUTERMOST FULL

POSITIVELY CHARGEDNEGATIVELY CHARGED

___________________________: FORM THROUGH THE ____________________________ BETWEEN

OPPOSITELY CHARGED IONS.

IONIC BONDS ELECTRICAL FORCE

Sodium atom (Na) Chlorine atom (Cl)

Na loses an electron to Cl

Ionic bondGained electron

Sodium atom (Na+)

Chlorine atom (Cl-)

The sodium atom loses its one outer electron to the chlorine atom.

The positive sodium ion and negative chloride ion attract each other and form an ionic bond.

•Two or more atoms held together by __________ _______.

•Smallest part of a ____________________.

•Almost all substances that make up organisms, (____________________________________________) are molecules held together by covalent bonds.

COVALENT BONDS

ELEMENT

LIPIDS, NUCLEIC ACIDS, WATER

Oxygen Atom (O) Oxygen Atom (O)Carbon Atom (C)

CARBON DIOXIDE (CO2):

Oxygen:

_____Protons, ___ Neutrons _____Electrons (6 outer/2 inner)

Carbon:

_____Protons, ___ Neutrons _____Electrons (4 outer/2 inner)

8 88

6 66

covalent bonds

6 C12

= OXYGEN = HYDROGEN

COMPOUND:

WATER = H2O

MOLECULES OF H2O = ______7

= OXYGEN = HYDROGEN

Practice:

How many water molecules will be created as a result of covalent bonds?

TOTAL MOLECULES OF WATER “EXTRA” ELEMENTS

OXYGEN HYDROGEN

___________ ___________ ___________7 2 1

= OXYGEN = HYDROGEN

More Practice:

How many water molecules will be created as a result of covalent bonds?

TOTAL MOLECULES OF WATER “EXTRA” ELEMENTS

OXYGEN HYDROGEN

___________ ___________ ___________11 0 4

1. Matter:

2. Atoms:

3. Elements:

4. Compound:

5. Molecule:

Anything that has mass and takes up space.

Made up of atoms.

Make up elements

Substances that are made up of only one kind of atomoxygen, hydrogen, carbon, nitrogen

Substances that are made up of two or more elementsWater, (H2O) , Carbon Dioxide, (CO2)

The smallest part of a compoundYou must have 2 hydrogen molecules and 1 oxygen to have WATER.

__________________________________________

____________

____________

____________

____________

____________

____________

_OTHER_____

____________

OXYGEN, (O)

CARBON, (C)

HYDROGEN, (H)

NITROGEN, (N)

CALCIUM, (Ca)

PHOSPHORUS, (P)

SULFUR, (S)

•Organisms’ bodies, (their _____________),

are made up of mostly ____________________

•The water in cells gives the cell _______________

and ___________________ materials within

organisms.

•All of the processes necessary for an

organism’s life take place within the

______________________________ of the cell

CELLS

WATER

STRUCTURE

TRANSPORTS

WATERY ENVIRONMENT

1. ______________________

2. ______________________

3. ______________________

1. HIGH SPECIFIC HEAT

2. COHESION

3. ADHESION

Negative Charge

Positive Charge Positive Charge

•Water is a “______________” molecule

•Form when atoms in a molecule have ____________ pulls on the _____________ they share.

•Opposite charges of polar molecules can interact to form ____________________ bonds.

•An attraction between a slightly _______________ hydrogen atom and a slightly ______________ atom.

(Usually _______________________________)

•Hydrogen bonds are part of the structures of _______________ and of ______________

Shared Electrons

POLAR

UNEQUALELECTRONS

HYDROGEN

POSITIVENEGATIVE

OXYGEN OR NITROGEN

PROTEINSDNA

• Hydrogen bonds give water an abnormally ____________________________.

•Water __________________ changes in temperature because it must _____________ more ____________________ to increase in temperature.

HIGH SPECIFIC HEAT

RESISTS

absorb more heat energy

Cohesion: the attraction among __________________ of the same substance.

Cohesion from hydrogen bonds makes water molecules _____________________.

Cohesion produces __________________, ( “skin on water” )

MOLECULES

STICK TOGETHER

SURFACE TENSION

Adhesion: the attraction among __________________ of ______________ substances.

For example, water molecules stick to other things.

Water in a test tube, (water is attracted

to the ____________)

MOLECULES DIFFERENT

GLASS

Materials such as ________________ and ____________ cannot be transported form one part of an organism to another unless they are dissolved in blood, plant sap, or other water based fluids.

______________: Mixture of a substance that is the same throughout.

___________: Substance that is present in the greater amount and dissolves another substance.

___________: Substance that dissolves in a solvent.

SUGARS

OXYGEN

SOLUTION

SOLVENT

SOLUTE

Some compounds form ______________ or _____________

because they _______________ into _______________

when they dissolve in ___________.

BASE: Compounds that

remove H+ ions

from

a solution

ACID: Compoundsthat releasea proton - a hydrogen ion(H+) – when it dissolves in water

ACIDS BASES

BREAK UP IONS

WATER

____________________

____________________

____________________

____________________

____________________

PROTEIN

LIPIDS

CARBOHYDRATES

ATP

NUCLEIC ACID

•USED BY CELLS FOR __________ ___________ AND __________ ____________.

SIMPLE CARBS = _______________________________

COMPLEX CARBS = _____________________________

_____________________________

ENERGY SOURCEENERGY STORAGE

ONE OR TWO SUGAR MOLECULES

LONG CHAINS OF SUGAR MOLECULES

Ex) Starches such as potato,

pasta, bread________________________________

________________________________

•MAKE UP _________________.

•INVOLVED IN ALL _______ ____________.

•BUILDING BLOCKS = _________ __________.

•_________________= TYPE OF PROTEIN THAT STARTS AND SPEEDS UP CHEMICAL REACTIONS IN CELLS.

CELLS

LIFE PROCESSES

AMINO ACIDS

ENZYME

•DON’T MIX WITH ______________.

•PHOSPHOLIPIDS – MAKE UP ________ ______________.

•FATS AND OILS THAT _________ ___________.

•ORGANISMS USE FATS AND OILS WHEN THEY HAVE USED UP ___________________.

•_________- SOLID AT ROOM TEMPERATURE.

•_________- LIQUID AT ROOM TEMPERATURE.

WATER

CELL MEMBRANE

STORE ENERGY

CARBOHYDRATES

FATS

OILS

•MAJOR ___________ ___________ MOLECULE IN CELL.

•ENERGY IN __________________ AND __________ AND _____________________ MUST BE TRANSFERRED TO ATP IN CELL TO BE USED.

ENERGY CARRYING

CARBOHYDRATES LIPIDS PROTEINS

•HAVE ALL INFO NEEDED TO MAKE __________.

•“_______________” OF LIFE.

•BUILDING BLOCKS OF _____________.

•TWO TYPES: ________ AND _______.

PROTEIN

BLUE PRINT

NUCLEOTIDES

DNA RNA

COMPOUND BUILDING BLOCK

(POLYMER) (MONOMER)

PROTEIN AMINO ACID

LIPID (FAT) FATTY ACID

CARBOHYDRATE SUGARS

NUCLEIC ACIDS NUCLEOTIDE