General Chemistry 1 Exam 1

Exam 1 p

physical change:

change that does not affect the substance

examples of physcia, change

breaking glass, folding paper

Chemical Change

change that does affect the composition

example of chemical change

oxidation, combustion, decomposition

Scientific notation

rewriting bug or small numbers more manageable

Density equation

D= m/v, density equeal mass over volume ,

usually keep 2 decimal places

Significant figures

how many decimal places should you report

Rules of sig figs

1. all numbers 1-9 are significant

2. sandwiched 0’s between numbers are significant

3. zeros at the end do count only if there’s a decimal

Adding/ subtracting sig figs

look at the number of decimal places, least amount is what we report

Multiplying and dividing sig figs

we look at least number of sig figs

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• Tera

• Giga

• Mega

• Kilo

• deci

• centi

• milli

• micro

• nano

• pico

Metric prefixes

• Tera- (1×10^12)

• Giga- (1×10^9)

• Mega- (1×10^6)

• King- (1×10^3)

• deci- (1×10^-1)

• centi- (1×10^-2)

• milli- (1×10^-3)

• micro- (1×10^-6)

• nano- (1×10^-9)

• pico- (1×10^-12)

Each elemetn is composed of

small particles (atoms)

Atomic number tells us the

amount of protons and electrons

mass # tells us number of

protons + neutrons

Protons and neutrons are in the

nucleus

mass of isotope equation

(mass)(%)+ (mass)(%)/ 100

isotopes

same # of protons (atomic number) but different number of neutrons (atomic mass)

Alkali metals

group 1

Alkaline earth metals

grouo 2

Transition metals

lowered part of periodic table

Chacogens

group 6

Halogens

group 7

Noble Gases

group 8

distinction between metals and nometals

division line

• positive metal (left)

• negative nonmetal (right)

Ions

cations and anions

cations

(+) metals

anions

(-) nonmetals

Covalent compound

2 or more nonmetals

use prefixes in what backround

covalent

prefixes

1. mono

2. di

3. tri

4. tetra

5. penta

6. hexa

7. hepta

8. octa

9. nona

10. deca

how to name covalent compound

Prexix- nonmetal prefix- 2nd nonmetal (ide)

• write formula how you read it

Binary Ionic formula

NO PREFIXES - metal first then nonmetal (ide)

Formula of Binary Ionci formula

swap and drop

Polyatomic

grouo if elements bonded together

Transition metals

charge of transiiton always given to you

Acids

a compound that can donate a proton , H in the front

Binary acids name

Hydro- nonmetal (ic) acid

Polyatomuc acids

ate if looses oxygen goes to it

• CO3 to CO2→ carponate to carbonite

Naming polyatomic acid

if ends it ate goes to ic

H2CO3→ carbonic acid

• if ends in ite gous to ous

H3CO2→ Carbonous acid

Molar Mass

mass of all elements added up in the compund

% composition

part/ whole *100

Stoichiometry

covert between grams (molar mass) <→ moles(6.022×10²³) ←> particles/molecules/atoms

Empirical formula

reduced formula

molecular formula

true formula

To find emperical formula

1. take whats given and convert to moles

2. divide all by smalles number

syntehsis reaction

A+B → AB

Dcompostion reaction

AB→ A+B

single replacement reaction

A+BC→ B + AC

double replacement reaction

AB+CD→ AD+ CB

combustion reaction

CxHy+O2→ CO2+H2O (ALWAYS)

to balance combustion. start with 2

Strong Electrolyte

a solution that has ions (cations and anions)(metal and nonmetal)

ex. NaCl

Strong Acids

1. HCL

2. HBr

3. HI

4. H2(SO4)

5. H(NO3)

6. H(ClO4)

concetration/ molarity equation

moles/liter = M

Dilution equation

M1*V1 = M2^V2

double replacement reactions

switch metals

single replacement

swith metals ONLY if single metal is higher on table

net ioninc equations

show reacting species

precipitate

product new portion that is a solid

Net ionic steps

1. Balacne Equation

2. break apart anything that is aqueous

3. cancel spectator ions

4. rewrite anything that remains

Redox reactions

reduction + oxidation occurs simultaneously

reduction

gaining of electrons

oxidation

looses electrons (OIL RIG)

Rules for determining oxidation

1. Alkaline metals +1

2. Alkine earth metal +2

3. Halogens (group)7 -1

4. Chalogens (group 6) -2

5. diatomics and single metals → 0

Diatomics

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1, Hydrogen

2. Nitorgen

3. Florine

4. Oxygen

5. Iodine

6. Chlorine

7. Bromine