Gen Chem Exam 1

 

 

Carbonate

 

 


CO3 -2

 

 

Hydrogen Carbonate 

 

 

HCO3

 

 

Nitrite

 

 

NO2  

 

 

Nitrate

 

 

NO3 – 

 

 

Phosphate

 

 

PO4 -3

 

 

Hydrogen Phosphate

 

 

HPO4 -2

 

 

Dihydrogen Phosphate

 

 

HPO4

 

 

Hydroxide

 

 

OH

 

 

Sulfite

 

 

SO3 -2

 

 

Sulfate

 

 

SO4 -2

 

 

Hydrogen Sulfate

 

 

HSO3 – 

 

 

Hypobromite

 

 

BrO

 

 

Bromite

 

 

BrO2  

 

 

Bromate 

 

 

 

 

BrO3

 

 

PerBromate

 

 

BrO4  

 

 

Ammonium

 

 

NH4 +

 

 

Acid formula starts with:

 

 

H

 

 

Base formula contains:

 

 

OH

 

 

A salt is:

 

The ionic product of an acid-base neutraliazation reaction.

 

 

CaO:

 

 

Calcium oxide

 

 

AlCl3:

 

 

Aluminum chloride

 

 

CuCO3:

 

 

Copper (II) Carbonate

 

 

Element:

Simplest form of matter, cannot be decomposed into simpler substances, made up of only one type of atom.

 

 

Compound

Made of elements, elements are always present in the same proportion, different properties from the elements that make it up

 

Types of compounds:

 

1. Ionic

2. Molecular

 

K = 

 

C + 273.15

 

 

1 mm = __ m

 

 

0.001 m

 

 

1 microgram = ___ g

 

 

10-6 g

 

 

1 nm = ___ m 

 

 

10-9 m

 

 

1 kg = ___ g

 

 

1000 g

 

 

1 dm = ___ cm

 

 

10 cm 

 

 

1 Mton = ___ ton 

 

 

106 ton 

 

 

1 L = ___ dm3 = ___ cm3

 

 

1 dm3 = 1000 cm3

 

 

Precision = 

 

 

repeatability

 

 

Accuracy = 

 

 

closeness to true value 

 

 

1 u = ___ g 

 

 

1.661 x 10-24

 

 

Atomic number =

 

 

the number of protons in the atom (an atom’s identity)

;

;

Mass number =

;

;

the number of protons and neutrons in an atom;

;

;

Isotopes =

elements made of the same atoms (same atomic number), but the atoms have different masses (different number of neutrons)

;

;

Atomic weight =;

the weighted average of all naturally occurring isotopes, this is the number shown on the periodic table

;

;

1 mol = _______

;

;

6.022 x 1023

;

;

1A

;

;

alkali metals;

;

;

2A

;

;

alkaline earth metals

;

;

6A

;

;

chalcogens

;

;

7A

;

;

halogens

;

;

8A

;

;

noble gases;

;

;

Empirical formula:

smallest whole number ratio of atoms in a compound

;

;

Molecular formula:

actual number of atoms in a molecule of the compound;

;

;

Structural/Condensed formulas:

show picture/give information on the structure of the molecules;

;

;

Molecular compound =;

nonmetal + nonmetal;

covalent bonds (share es)

no charges involved

can’t always predict formula

 

 

Ionic compound = 

metal + nonmetal

cations + anions

ionic bonds (electrostatic attrctn)

3D structures

 

 

 

Acid produces __(aq) in water:

 

 

H+ (aq)

 

 

Base produces ___(aq) in water:

 

 

OH(aq)

 

 

-ide to      acid 

 

 

hydro__ic acid

 

 

-ite to    acid 

 

 

___ous acid 

 

 

-ate to       acid 

 

 

____ic acid 

 

 

molecular formula = x/y times z

 

 

= molecular weight/empirical weight x empirical formula

x

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