Chem 1/2/3/4

how many cm in an in

2.54 cm in 1 in

how many kg in 1 lb

2.205 lb in 1 kg

how many mL in L

1000 mL in 1 L

how many m in km

1000 m in 1 km

what is a J

10^(-15)

how many mg in g

1000 mg 1g

how many mL in cm

1 mL in 1 cm

how many km in 1 mi

1.61km in 1 mile

kilo (k)

10³

deci (d)

10^-1, 0.1m

centi ©

10^-2, 0.01m

milli (m)

10^-3, 0.001m

micro (M)

10^-6, 1×10^-6m

boiling point C

100 C

freezing point C

0C

room temp C

25 C

how many ML in 1 cm

1mL=1cm³

1cm³ Volume

1×10^-6m³

1dm³ volume

1×10^-3m³

1L=1000mL=?

1000cm³=1dm³

water formula

H2O (l)

ammonia formula

NH3 (g)

methane formula

CH4 (g)

Isotope Formula

weighted average=(#1 natural abundance%)(individual mass)+(#2 natural abundance%)(individual mass)

NH3 (aq) what is the base

base, aqueous ammonia

md substance

gramsx/mm (grams-ions, compounds)

Have No Fear Of Ice Cold Beer

H(g), N(g), F(g), O2(g), I2(s), Cl2(g), br2 (l)

how to convert F to C

K=C+273.15

273.15k=0C

373.15k=100C

F=9/5xC+32

32F = 0C

212F = 100C

area of cirlce

(pie)r²

sphere volume and area

area=4(pie)r²

volume=4/3(pie)³

cube area and volume

area=6a²

volume=a³

how many m in cm

1m=10²cm

what is the Si unit in kg and m

Si unity is kg/m³

density fractions (3)

mass/volume; volume=m/d; m=d.v

% error formula

(average experimental value)-(true value)/(true value) x100

daltons atomic theory

elements that are small-atoms

all atoms are identical

compounds definition

atoms, more then 1 element, ratio is integer/simple fraction

chemical reaction

seperation, combonation, rearrangement does not result in creation

whats in an atom

protons, neutrons, electrons

protons mass/charge

mass=1.67×10^-10

(+)

in nucleus

neutron mass/charge

mass=1.0086

neutral charge

in nucleus

electron mass/charge

mass=5.485×10^-4

negative charge

around nucleus

molecule

2+ atoms held together

ex) H20

diatomic molecule

2 atoms

polyatomic molecule

more then 2 atoms

which comes first in a molecular formula

furthest to the left, closest to bottom is first

ion

positive and negative charge

cation

+ looses election, p stays same

anion

- gains electron, p stays same

ionic compounds

cations and anions

formula must =0

metal and non metal

hydrates

compounds that have specific number of water molecules attached

what is C conversion

1 mole 12.001g

s 1 mole= 32.00g

molecular mass in moles

mm=grams of C/12.01. =gramsx/mm

how many groups in the periodic table

18

how many periods in the periodic table

6

main group elements

1-2, 13-18

group 1

alkali metals

group 2

alkali earth metals

group 7

halogens

group 8

inert gass

where is the most metallic on the table

to the left bottom

where are cation and anions

cation- left

anion-right

prefixes

1-mon

2-di

3-tri

4-tetra

5-penta

6-hexa

7-hepta

8-octa

9-nona

10-deca

rules of balancing equations

1-balence carbon

balance H next

3-balence O last

nobel gasses

right side, group 18, lack of chemical reactivity

inert gasses

least reactive

lanthanide series #s

57-71 at bottom, compact table

actinide series #s

89-103

semimetals/metalloids

brittle, solids, not conduct electricity,

transition metal #

13-21, nonmetallic, high density

organic compounds

contains carbon, complex

diagonal relationships

similarities in reactivity between first element ini aa group and second in the following

how many J in kJ

10³J=1KJ

how many mJ in 1 J

10³mJ=1J

how many aJ in 1J

1J=10^-18aJ

what are the charges with X

X is (X+)+e-

X+ is (X2+)+e-

X2+ is (x3+)+e-

x is x3+3e-

charges in IE

IE1<IE2<IE3

elements with low ionization energy

cations, metals, conduct electricity

elements with high ionization energy

anions, nonmetals, no energy

valence electrons

low ionization, outer most shell, easy to move

core electrons

never leave, held tight in nucleus

lambda

wave length, nano meters

how many nm in 1m

1nm in 10^-9m

nu V

frequency

nu equation

c/lambda

speed of light equation

c=3.00×10^8 m/s

frequency of green

c=landum/nu

colors of energy from low to high

high R, O, Y, G, B, P low

what is c

speed of light, 3.00 × 10^8 m/s

what is s-

5.50× 10^14

emission of an atom

high E-high frequency(nu)-short wave length (lambda)

low E-long frequency(nu)-long wave length(lambda)

energy state

region with all the energy

ground state

lowest energy level (not zero)

absorption

arrow up, nf on top, ni on bottom, (+), light absorbed

emission

arrow down, ni on top, nf on bottom, (-), light emitted

rydberg

know how to calculate energy

photon

bundle of energy

photoelectric effect

light has both wave,

hv=KE+W

KE=hv-W

what is w in light waves

w is work function, how strong electrons are

what is v in light waves

threshold frequency (depends on metal)