CHEMISTRY OF LIFE 1. Matter: a. All matter takes up space and has mass b. All living and nonliving matter are made up of elements c. Elements are pure and are naturally occurring * elements cannot be broken down into substances with different chemical or physical properties. 2. Six elements make up 98% of all living things C= Carbon, H=Hydrogen, N=Nitrogen, O=Oxygen P=Phosphorus, S=Sulfur 3. Compounds: 2 elements bonded together.
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CHEMISTRY OF LIFE 1. Matter: a. All matter takes up space and has mass b. All living and nonliving matter are made up of elements c. Elements are pure.
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CHEMISTRY OF LIFE1. Matter:
a. All matter takes up space and has mass
b. All living and nonliving matter are made up of elements
c. Elements are pure and are naturally occurring
* elements cannot be broken down into substances with
different chemical or physical properties.
2. Six elements make up 98% of all living things
C= Carbon, H=Hydrogen, N=Nitrogen, O=Oxygen
P=Phosphorus, S=Sulfur
3. Compounds: 2 elements bonded together.
CHEMISTRY OF LIFE CON’T
Elements: Pure substance, only 1 kind of atom. Represented by a letter: O , N, P Or two letters: Mg, Cu, Li
Compound: Two elements bonded together.
Ex: NaCl, H2O
Molecular Formula: Tells you how many atoms of each element in a molecule.
Structural Formula: graphical representation of the molecular structure, showing how the atoms are arranged
CHEMISTRY OF LIFE Atoms: smallest unit of matter that cannot
be broken down any further. a. Electrons: negative charge (e-) Outside
b. Protons: Positive charge (p+)
c. Neutrons: no charge (n) Inside the Nucleus
Atomic Number=Number of protons
Number of Protons=Number of Electrons
WHY BOND TOGETHER? 1. Arrangement of Electrons! Grouped into different levels Inner levels have more energy than outer levels. Outer levels must have a certain number of electrons in
it. If not, it is considered unstable and will react with other elements to help it have 8 in its outer shell becoming stable. (You will learn in chem that there are some levels that can hold more than 8. But for our purposes we are going to keep it at 8)
E1= 2
E2= 8
E3 = 8
ELECTRON DOT EXAMPLE
Cl
# of Protons= Atomic Number = 17
# of protons = # of electrons = 17
# neutrons = Atomic number – Atomic Mass
17 - 35.453 = 18
TYPES OF BONDS Covalent: When two or more atoms are shared between
elements.
Example H2O
IONIC BONDING
Ionic: When elements gain or lose electrons: creates a charge
a. If lose an electron: positive charge
b. If gain an electron: negatively charged
c. This charge difference is what attacks the two elements
HYDROGEN BONDING
Attraction between a partial positive and partial negative charge molecule. Partial negative charge is oxygen, fluorine, or nitrogen and partial positive charge is hydrogen
Special bonding between water
Link to animation of Hydrogen Bonding in Water - Northland Community and Technical College http://www.north
land.cc.mn.us/biology/Biology1111/animations/hydrogenbonds.html Weaker than covalent and ionic bonds Nonpolar: equal charge: do not like water Polar: Unequal charge: water liking