IHS Chemistry

gas, liquid, solid, plasma

it possesses neither shape nor volume, expands indefinitely

they possess volume and assume the shape of their container

They possess volume and shape. They cannot be compressed.

mixture of ionized gas and free-floating electrons

• molecular activity
• dictated by heat and pressure

its atoms

a pure substance that cannot be broken down into simpler substance by chemical reactions

• 1) all matter is made up of tiny particles called atoms
• 2) all atoms of the same element are identical
• 3) atoms of one element are different from another element
• 4) atoms combine to form molecules

a pure substance of 2 or more elements in a FIXED PROPORTION by weight

a combination of elements and compounds (ex: room air)

a tightly chemically bound group of atoms

• powerful attraction that holds atoms together
• 1) ionic
• 2) covalent

atomic weight increases

• they are in the same column
• they share chemical and physical properties

within the nucleus

number of protons in the nucleus

the weight of the protons and neutrons in the nucleus

2, 8, 8

inert

carbon, oxygen, hydrogen, nitrogen

Ferrous (Fe +2)

Bromine 35

Calcium 20

Carbon 6

Chlorine 17

Fluorine 9

Helium 2

Hydrogen 1

Iodine 53

Iron 26

Nitrogen 7

Oxygen 8

Potassium 19

Sodium 11

Sulfer 16

• a particle with an unequal number of protons and electrons
• cation (+)
• anion (-)

the attraction between positive and negative ions. strongest of the electrostatic bonds.

metal and non-metal

the greater the charge, the greater the attraction

• 1) dipole-dipole
• 2) hydrogen bonding
• 3) london forces

the attraction between the oppositely charged ions of polar molecules

The bond between an ion and a polar molecule

a special type of ion dipole bond that occurs when hydrogen is bound to N, O, or F

An instantaneous pole that is created whenever electrons in a molecule are unevenly distributed.

results from SHARING one or more pairs of electrons

the covalent bond

CH4

CH3

Any group of atoms that have bonded together to act like an individual atom in chemical reactions

SO4 2-

NO3-

PO4 3-

CO3 2-

OH-

HCO3-

NH4+

4

3 or 4

2

1

2, 4, or 6

1

1

1

1

2 carbons, 6 hydrogens (all single bonds)

3

4

5

6

7

8

9

10

includes a double bond

includes a triple bond

compounds that have identical molecular formulas but several alternate structures

it has the unique ability to rotate its bonds around its central axis

• 1) Structural - differ in physical and chemical properties, same components, just arranged differently
• 2) Stereoisomer - identical formulas but differ in their spatial arrangement. (2 types: optical and geometric)

• when carbons atoms differ from on another in such a way as to polarize the light
• - to the right = dextroisomer
• - to the left = levoisomer
• - mirror images

combine dextro and levo isomers so that no bending of light occurs

• when a double bonded carbon prevents axial rotation so the R's move
• - cis isomer (R's on same side)
• - trans isomer (R's on opposite sides)

a set of atoms bound together in a specific way - responsible for the chemical and physical properties of a compound

• - functiontional group is a halogen (F, Cl, Br, I)
• - generic formula is R-X

• - two radical groups joined by an atom of oxygen
• - oxygen is the functional group
• - generic formula: R-O-R

• - alcohol + acid
• - generic formula: R-COO-R

• - related to carboxylic acid
• - generic formula: -CONH2

• - functional group is the nitrogen atom
• - generic formula: R-NH2
• - can be divided into primary, secondary, tertiary depending on how many of the hydrogen atoms are replaced by a radical
• - derivative of ammonia (NH3)

• - proteins or peptides
• - amines or amino acids
• - steroids

sympathomimetic amines

- 6 carbon ring with 3 double bonds

-OH

CH3

NH2

HC - CH3 - CH3

methylation of the terminal amine