1. Chemistry of Life
Matter

2. Matter Makes up everything
Matter is anything that has mass and takes up space (volume)
Basic unit of matter is the atom.

3. Atoms
Atoms are the smallest unit of matter made of protons, neutrons and electrons.
Atoms have very specific properties that make them the building blocks of everything we know.

4. Atoms
Electrons- are small (1/2000 in mass to a proton and neutron) negatively charged particles found around orbiting the nucleus in the electron cloud.
Protons- are positively charges subatomic particles that are located in the nucleus
Neutrons- are neutral in charge, subatomic particles found in the nucleus

5. Atoms, Elements, and Isotopes
Atoms of the same type are called elements.
Elements are placed together in a collection on periodic table
Elements on the periodic table are organized by their properties
These SIX are MAJOR elements that make up living things
Sulfur (S), Phosphorus (P), Oxygen (O), Nitrogen (N), Carbon (C), Hydrogen (H)
SPONCH

6. The World of Elements Different kinds of atoms = elements H C N O NaMg P S K Ca
Different kinds of atoms = elements

7. Atoms, Elements, and Isotopes
Other elements that make up living systems are Calcium (Ca), Sodium (Na), Magnesium (Mg) and Potassium (K)
All elements are given a name and a symbol. The symbol may appear to not match up with its name but that is because the symbol is from its Latin name.

8. Properties of Atoms
The number of protons is equal to the number of electron in a neutral atom
Carbon has 6 protons which means it will have 6 electrons
If the number of protons change then the identity of the element changes
Identify that element
20 Protons
11 electrons
92 electrons
17 protons
26 protons Ca Na
Uranium Cl
Iron, Fe

9. Periodic Table
Each element has a box of information on the Periodic Table.
Atomic number (# or protons)
Atomic mass
Symbol of the element
Name of the element

10. Elements form Compounds
Compounds are substances formed by chemical combination of 2 or more elements in definite proportions. Compounds are represented by chemical formulas CO CO2

11. Elements form Compounds
Compounds always have different properties than the elements that make them up. Table salt is NaCl Na is sodium which is very reactive. Cl is chlorine is a toxic gas. When the two combine they form a compound that can be ingested.

12. Elements form Compounds by chemical bonds
Chemical bonds are interactions between two elements electrons
The electrons involved in bonding are called valence electrons
TWO TYPES of BONDS:
IONIC BONDS
COVALENT BONDS

13. Ionic Bonds
Bonds that are formed when 1 or more valence electrons are transferred from one atom to another.
Ionic bonds form between ions
Ions are atoms with a charge

14. Ions
Positively charged ions are the result of an atom losing electrons (e-) A positively charged ion is called a CATION.
Negatively charged ions are the result of an atom gaining electrons (e-) A negatively charged ion is called an ANION.

15. Covalent Bonds Bonds that are formed when two atoms “share” electrons
When electrons are shared the compound is called a MOLECULE
Water is a molecule
H2O

16. Why do elements bond?
Each element wants 8 electrons in its highest energy level.
This can only happen when elements bond with each other
The 8 electrons are referred to as an OCTET.

17. Other Forces
Van der Waals Forces are forces between molecules (intermolecular forces)
These forces link one molecule to another

18. Intermolecular Forces
All elements are not created equal. In covalent bonds some elements have a stronger pull on the electron over the other element.
Uneven pull creates area of charge on the molecule
Negative
Positive

19. Van Der Waals Forces Named after their discovery
Weak attractions between molecules
EXAMPLE: Geckos use Van der Waals forces to climb.
Van der Waals forces create attractions between the gecko’s foot and the surface on which it is climbing.