Chemistry & Carbon

The Cellular Basis of Life

Atomic Structure Elements: smallest unit a substance can

be broken down into and still have the same chemical properties1. 92 naturally occurring elements2. 25 of the 92 are essential to life3. carbon, nitrogen, hydrogen, & oxygen

are important4. trace elements are required by an

organism in very small amounts

Atomic Structure Continued

Atom: smallest form of an element, made up of ….

1. proton – positive charge; in nucleus 2. neutron – no charge; in nucleus 3. electron – negative charge; outer

energy level (only 2 e-’s can occupy the same orbital)

Atomic Structure

Compound: 2 or more elements combined in a fixed ratio

Atomic Number: # of protons Mass Number: # of protons + # of

neutrons Isotopes: atoms of the same elements

with different numbers of neutrons Ion: negatively charged particle

Bonding & Electrons

Atoms want to fill their outer energy level to b/c stable

Electrons have energy the further from the nucleus, the more energy e-’s have

As e-’s move to higher energy levels, energy is ADDED to them

As e-’s move back down energy levels, energy is LOST or RELEASED

Chemical Bonding

Types of Chemical Bonds

Ionic Bond Covalent Bond

HydrogenBond

Non-polarCovalent

Bond

Polar Covalent

Bond

1) Ionic Bonds

Definition: attraction of oppositely charged ions;

Lose and gain electrons Ex. Na+ + Cl- NaCl The Na+ gives up one electron & the

Cl- gains one electron Easier to break than covalent bonds

1) Ionic Bonds

2) Covalent Bonds

Definition: two atoms share electrons; strong bond Non-polar Covalent Bond: electrons

are shared equally Ex. Hydrocarbon chains

2) Covalent Bonds Continued

Polar Covalent Bonds: electrons are shared unequally due to electronegativity; strong bond Ex. Water

3) Hydrogen Bonds Definition: when electrons b/w hydrogen and

other atoms are shared unequally Hydrogen has a partial positive charge Hydrogen is attracted to slightly negatively

charged atoms Advantage: briefly together, respond & separate

4) Van der Waals Interactions

Definition: weak electric forces that attract neutral molecules to one another; Ex - A non-polar molecule with areas that

are positively and/or negatively charged These areas allow them to “stick” to

another molecule or area of a molecule

Weak force

Weak Bonds Examples of Weak Bonds are:

1. Hydrogen2. Ionic3. Van der Waals Forces

Advantage is….1. Holds a 3-D molecule in it’s correct shape2. may form b/w molecules 3. may form b/w regions of a single molecule

Strong Bonds

Examples of strong bonds are:1. Polar covalent 2. Non-polar covalent

Advantage is….1. bonds do not easily break2. these bonds hold together living

organisms in adverse situations

Carbon & Organic Chemistry Carbon 6

protons, electrons, & neutrons

What type of bond will it form? Why?

Carbon always wants to have ____ bonds

Other elements

Element # of Bonds

Nitrogen

Oxygen

Hydrogen

Types of Isomers

Structural Isomer: differ in structural arrangement of their atoms

Geometric Isomer: differ in spatial or 3-D arrangements

Stereoisomers: mirror images of each otherEx. Thalidomide

Structural Isomer

Geometric Isomer

Stereoisomer

Functional Groups & Behavior

Chemical groups attached to the carbon skeleton of a molecule Determine the “behavior”or properties of

the molecule Ex – Hydroxyl =‘s polar behavior = will

bond with other polar molecules Ex – Methane =‘s nonpolar behavior =

will bond with other nonpolar molecules

Functional Groups

Functional Group Formula

Hydroxyl or Alcohol -OH

Carboxyl -COOH

Amino -NH2

Ketone & Aldehyde -CO & -CHO

Phosphate -PO4

Sulfhydryl -SH

Monomers Link to Make Polymers

How are Polymers Made from Monomers?

Dehydration Synthesis Aka, condensation reactions Links monomers together by removing water H (from one monomer) and OH (from another

monomer combine to form water

How are Polymers broken back down into monomers?

Hydrolysis Breaking a polymer into many monomers

by adding water

Dehydration Synthesis & Hydrolysis