Inorganic Analysis

I. Matter- made of mass and volume

A. Atoms- smallest unit of matter

1. Nucleus- center of atom

a. Neutrons- neutral charge, 1 amu
b. Protons- positive charge, 1 amu

2. Electrons- orbit the nucleus, -1 charge, 0 amu

a. Electrons are located around the nucleus and arranged in energy levels (shells)
b. Energy levels

i. K = 2 electrons
ii. L = 8 electrons
iii. M = 8 electrons

B. Elements- same kind of atom, approximately 110 elements

1. Symbols- shorthand of elements

2. "Fingerprint" is obtained by emission spectroscopy; similar to flame test

3. Oxygen is the most abundant element in the earths crust

C. Compounds- 2 or more kinds of atoms that are chemically combined

1. Emission Spectrograph is used to determine elemental composition of a substance.

D. Atomic Number- the # of protons of an element

E. Atomic Mass- weight of the atom, the number of protons plus the number of neutrons

F. Isotopes- an element that has the same number of protons but different number of neutrons

1. Radioisotopes are isotopes that have unstable nuclei

a. Emit particles or energy from the nucleus

b. Neutron activation analysis identifies an element by measuring the energy of gamma rays

ex.)gamma rays are a form of electromagnetic radiation

c. Examples: hydrogen, deuterium & tritium

2. Tracers- the use of isotopes to study biochemical reactions

II. Chemical Bonding

A. Ionic Bonds

1. In an atom, the number of protons equals the number of electrons and therefore, the atom is neutral
2. Ion- an atom that has lost or gained electrons (to complete the outer shell) and now has a charge (charged particle)
3. Ionic bond is the transfer of electron(s) from one atom to another to form a neutral compound (NaCl, CaCl, LiF)
4. Crystalline substances are identified by x-ray diffraction

B. Covalent Bond- a compound formed from the sharing of electrons

1. Diatomic molecules- a bond formed from 2 atoms of the same element (H2 O2)

III. Chemical Reactions

A. Chemical formulas- every compound consists of atoms in definite proportions

1. Molecular formula- shows the symbol of elements and how many atoms of each are present (H2O, C6H12O6)
2. Empirical formula- show the symbol and atoms in lowest ratio (CH2O)

B. Chemical Equations- chemical bonds are broken and new products are formed

1. The number of atoms of each kind of the reactants must equal the number of atoms of each kind on the product side

IV. Mixtures- made up of substances that are not chemically combined; therefore, retain their own individual properties (salad, salt water)

A. Solutions- homogeneous mixture (same phase), particles do not settle out

1. Solvent- dissolving agent
2. Solute- substance being dissolved

B. Suspensions- substances settle out of the liquid (mud)

C. Colloids- a suspension in which the particles do not settle out (foam, cream,
mayonnaise)

V. Acids- compounds that donate a hydrogen ion (H+), have an J in front of their formula

A. Sour taste, corrosive
B. In H2O, acids separate into its ions

VI. Bases- compounds that accept H+, contain a hydroxyl group (OH)

A. Bitter taste, slippery (lye)
B. In H2O, bases separate into it ions

VII. Neutralization- when solutions of acids and bases are mixed, water and salt are formed

VIII. pH Scale- a scale based from 1-14

A. 1-6.9 acids (lower numbers being stronger acids)
B. 7 neutral (water)
C. 7.1-14 bases (higher numbers being stronger bases)

IX. Indicators- a substance that changes color when the pH goes above or below a certain value
ex) blue litmus paper, red litmus paper, methyl orange, phenolphthalein

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