“…beneath the clothes, we find a man... and beneath the man we find... his... nucleus.”-Nacho Libre

 The structure and function of all living things are governed by the laws of chemistry.  All organisms are made of matter.  Matter is constantly being rearranged through chemical reactions.

 Respond to the following in your notebook: If we continue to break things apart, eventually, will there be nothing left?

Living things (organisms): -Made of cells -Grow -Reproduce -Have DNA -Use energy -Need food

What do living and non-living have in common? All things are made up of matter.  Matter-anything that takes up space and has mass (solids, liquids, gas, plasma).

MASSWEIGHT Amount of matter an object is made of Pull of gravity on an object EXAMPLE: On the moon, your mass would be the same! Your weight would be different…less gravity to pull on your mass. Earth weight = 150 lbs Moon weight = 25 lbs Mass = 56g

element An element is:  A pure substance that cannot be broken down chemically into simpler kinds of matter. 4 Major elements:  oxygen,  hydrogen,  nitrogen,  carbon Approximately 90% of the mass of living things is made up of these four elements

Elements are arranged according to the number of protons they have.

element  Each element has unique chemical symbol ◦ Consists of 1-2 letters ◦ First letter is always capitalized

Atom-Simplest particle of an element that retains all the properties of that element.  Properties of atoms determine the structure and properties of the matter they compose.

1. Protons2. Neutrons3. Electrons Protons (in nucleus) Neutrons (in nucleus) Electrons Charge Positive (+) Neutral (no charge) NEGATIVE (-) MassBig VERY small

Nucleus Nucleus-central core of the atom, consisting of protons and neutrons. Electrons Electrons are found moving very fast around the nucleus in orbitals (electron cloud/energy levels).  Atoms with no charge (neutral) have equal protons and electrons.

DRAW A PICTURE OF AN ATOM (LABEL ALL THE PARTS)

Empty Space!!!

Atomic Number Atomic Number - # of protons in an atom (also tells the # of electrons). Atomic Mass # Atomic Mass # - number of protons + number of NEUTRONS **LABEL THE DIAGRAM**

compound A compound is:  Atoms of 2 or more elements chemically joined; the proportion is always fixed.  Also known as a molecule (2 or more atoms chemically joined). Example: H 2 O, O2, CO 2,

1. Share electrons2. Steal electrons Covalent Bond Ionic Bond Sa lt- the outer electron of Na atom is transferred to the Cl atom ~this results in ions - an atom with a + or – charge. Because + and – attract, this attraction is called an ionic bond.

Atom of OxygenMolecules of OxygenCompound containing Oxygen

In your notebook, respond to the following: On the Periodic Table locate the following elements and give the correct information: Atomic #, Mass, # Neutrons, # Electrons  Fluorine  Neon  Helium

It is the flow of energy that the Biologists seek to understand when they study the chemistry of living things…

Energy in Living Things: As energy flows through a living organism, it is converted from one form to another.

Atoms and molecules are in constant motion (kinetic energy). Amount of movement determines the state of matter. States of Matter 1. Solid 2. Liquid 3. Gas

 Particles linked together  Has a definite shape  Particles vibrate (little kinetic energy) Example: ice  Particles not as tightly linked.  Can flow, conform to the shape of the container.  Definite volume, not definite shape. Example: water

 Particles moving rapidly (lots of energy)  Fill volume of any container.  No fixed volume or shape Example: steam (water vapor) ***To cause a substance to change state, thermal energy (heat) must be added to or removed from a substance***

 Watch this video on Chemical Reactions at home!Chemical Reactions

Chemical Reaction-breaking or forming chemical bonds. Chemical Equation-represent chemical reactions; reactants are shown on the left, products are shown on the right. - Na + Cl ----  NaCl Reactants Products This chemical reaction is breaking chemical bonds, rearranging and forming new bonds …

Chapter 3-1 (pgs 49-51) Biology The chemical reactions of life, for the most part, occur in water solutions...

 The chemical reactions of all living things take place in an aqueous environment.  Water’s unique properties make it one of the most important compounds found in living things.

 Respond to the following in your notebook: Which one is more important, food or water?

three A water molecule (H 2 O), is made up of three atoms --- one oxygen and two hydrogen. H H O H

 POLAR COMPOUND-a compound where one end is more positively charged while another end is more negatively charged. oxygen atom attracts more electrons  In each water molecule, the oxygen atom attracts more than its "fair share" of electrons oxygennegative  The oxygen end “acts” negative hydrogenpositive  The hydrogen end “acts” positive neutral Zero Net Charge  However, Water is neutral (equal number of e- and p+) --- Zero Net Charge

 Polarity  Polarity makes water very good at dissolving things (effective solvent).  Water molecules attract other water molecules and solid surfaces. gy/Biology1111/animations/dissolve.html

 Water forms hydrogen bonds with other water molecules. ◦ HYDROGEN BOND ◦ HYDROGEN BOND-bond between hydrogen of one molecule and the negative region of another molecule. Cohesion and Adhesion ◦ Causes water to cling to itself and other surfaces: Cohesion and Adhesion

 COHESION  COHESION-the same kind of particles being attracted to each other (water sticking to other water). surface tension- ◦ Results in surface tension- a surface film on water that allows insects to walk on the surface. ◦ Causes water to be a very stable environment.

Surface Tension…this water strider cannot generate enough force to break through the hydrogen bonds of the water molecule !

 ADHESION  ADHESION-water molecules and molecules of solid surfaces are attracted to each other. ◦ EXAMPLE: water sticking to plant leaf

adhesion and cohesion  Together, adhesion and cohesion enable water molecules to move through narrow tubes against the force of gravity Capillarity (capillary action) Capillarity (capillary action)-the ability of water to move through fine pores or up a narrow tube against gravity due to adhesion  Example: the flow of water through its stem

A picture of Hydrogen bonds!

Adhesion Also Causes Water to … Form spheres & hold onto plant leaves Attach to a silken spider web

Capillary action (capillarity) Which gives water the ability to “climb” structures.

 Homeostasis - Ability to maintain a steady state despite changing conditions  Water is important to this process because: a. Makes a good insulator b. Resists temperature change c. Universal solvent d. Coolant e. Ice protects against temperature extremes (insulates frozen lakes)

 On a separate sheet of paper, answer the section review questions 1- 6 in your text on page 51.  All answers should be in complete sentences.

Mixture Mixture-substances are combined, but both keep their original chemical properties. ◦ Two Types:  Solutions  Suspensions

Solution Solution-a mixture where one or more substances is evenly distributed in another substance.  Aqueous Solution  Aqueous Solution-water is the solvent ◦ Made of 2 parts: 1. Solute-substance being dissolved in the solution. 2. Solvent-substance in which the solute is dissolved.

Concentration -Concentration-measure of the amount of solute dissolved in a fixed amount of solution. -More solute = greater concentration Saturated solution-no -Saturated solution-no more solute can be dissolved.

Substances that don’t dissolve, but separate into tiny pieces.  Example: sand in water, dust in a high wind.  The particles are large  Blood  Blood - red and white blood cells suspended in plasma  motion of blood keeps the cells from settling out

A mixture with particles larger than a solution, but the particles do not settle out.  Can exist as a gel  Example: cytoplasm

Solutions are either Acids or Bases

-pH 0-6 -Taste sour -Corrosive (burn things, eat away at materials *Acid rain can corrode stone and make bodies of water uninhabitable for life. Example: lemon juice, coke, vinegar, stomach acid.

-pH Bitter taste -Feels slippery -Corrosive *Also called alkaline* Example: ammonia, milk of magnesia, egg white

-Measures how acidic or basic a solution is. -From 0-14 Acids Bases

-Neither acidic or basic -pH = 7 Example: water

 Weak acids or bases that react with strong acids or bases to prevent sharp, sudden changes in pH (neutralization).  Produced naturally by the body to maintain homeostasis