Ba

1
Ba
Si
C
CHe
mistry
2
3
2
B H H SO
2
6

O
H
3
CH OH
2
4
H O
3
2
2
2
Introduction

• Laws of chemistry govern the structure and
  function of all living things!

3
Atoms

• a. simplest part of an element that retains all
  the properties of that element
• b. determine the behavior of matter
• c. subatomic particles
• protons (p) positively charged particles
• neutrons (nº) no charge
• electrons (e-) negatively charged particles

make up 99 of the mass
d. Net electrical charge of an atom is zero
because the number of p e- e. e- located in
orbitals (3-D space surrounding atom) 90 of
time f. Electrons are the only particles
involved in chemical reactions.
4
Orbital Shells
Bohr Model
H
a. valence electrons e- in outermost
shell b. valence shells are complete
(happy) when full c. 1st orbital 2 e- 2nd
orbital 8 e- 3rd orbital 8 e- 4th
orbital 16 e-
C
H
H
H
methane CH
4
1st shell maximum of 2 electrons
nucleus
2nd shell maximum of 8 electrons
3rd shell maximum of 8 electrons
4th shell maximum of 16 electrons
5
Matter
Solid

• Everything in the universe is made of matter.
• Anything that occupies space and has mass.
• Building blocks atoms
• Properties
• mass quantity of matter
• volume amount of space occupied
• density mass/volume
• weight pull of gravity

Liquids
Strong bonds
Weak bonds
Gas
Plasma
electron
-

No bonds


-
proton
Ionization
Phases of Matter
6
Forms of Matter

• a. element pure substance made of only one kind
  of atom
• cannot be chemically broken down into other
  substances
• over 100 elements, but less than 30 support life
• Carbon Hydrogen Oxygen Nitrogen
• (more than 90 of the mass of living things is
  made of these four elements)

6 C Carbon 12.0107
1 H Hydrogen 1.00794
8 O Oxygen 15.9994
7 N Nitrogen 14.00674
7
b. Compound two or more elements in a fixed
ratio Examples H O, CO , NaCl
2
2
Chemical formulas
ratio of water 2 hydrogen atoms to one oxygen
atom
c. Molecule simplest part of a substance that
retains all the properties of that
substance
d. Both represent different combinations of
atoms.
O - one type of atom
H O more than one type of atom
2
2
Forms both a molecule and a compound
Forms a molecule but not a compound.
8
Periodic Table of Elements
a. Atomic Number (unique for each element)
of protons in the nucleus of electrons in a
neutral atom b. Atomic Mass of protons
and neutrons in the nucleus
Mass number
13 protons AND 14 neutrons
27
Al
6 C Carbon 12.0107
13
Atomic number
Chemical symbol
Atomic number
13 protons OR 13 electrons
Name
Atomic Mass
9
Ion
SPECIAL ATOMS

• a. atoms that gain or lose electrons
• b. have an unequal number of p and e-
• c. have net negative or positive charge
• d. very reactive atoms

Na
Cl
Na
Na

sodium ion Na
sodium
10
Isotopes
(SPECIAL ATOMS)
6P 6N

• a. atoms with the same number of protons but a
  different number of neutrons different mass
• b. unstable nucleus releases radiation can
  damage living tissue
• c. Used in medicine and research
• 1. biological tracers
• 2. dating objects
• 3. treating cancer

Carbon 12
6P 8N
Carbon 14
11
Formation of Compounds by Bonding

• a. compounds have 2 or more elements in a fixed
  ratio
• b. have new properties from atoms
• c. covalent bonds 2 atoms share one or more
  valence electrons (forms molecules) very strong
  bond
• d. ionic bonds transfer of electrons formed by
  electrical attraction between two oppositely
  charged ions (forms crystals)