Chemistry Flashcards

the study of matter, its composition, properties, and transformation

Mass and occupied space.

rocks, minerals, everything of our crust

Hard? Soft? Density?

boiling, freezing, and melting point

involves into a new substance "transformation"

unique set of characteristics that identify a matter

L- Loose packed

H- Tightly packed

-1

-2

-3

-6

-9

-12

-15

3

6

9

12

independent of the quantity of matter ( color, odor, density, temperature)

dependent on the quantity of matter ( mass, volume, heat)

- non- zero digits are always significant

- any zeros between two sig digits are sig

- a final zero or trailing zero in the decimal portion are signfigant

- count the number of sig. figs in the decimal portion in the problem

- add or subtract

- round the answer to the last number of places in the decimal portion

- the least number of sig. figs in the problem is the number who determines the answers sig. figs

how much matter is in an object

refers to the force of gravity on an object

summarize all scientific observations about matter

smallest particle of an element that has properties of that element and can enter into a chemical combination

-discovered by democritus- believed atmons are made of particles that could not be broken down

consist of two or more atoms joined together by strong forces called chemical bonds

constant composition, pure ( nacl, h20,)

is composed of two or more types of matter that can be present in varying amounts and can be separated by physical change ( evaporation)

a mixture that varies from point to point ( sand water)

the properties of each substance don't change

also called a SOLUTION, exhibits a uniform composition and appears visually the same throughout

(Sports drinks).. same amount of sugar to water throughout ever drink

how close to the measurement is to the true value

is how consistent results are when measurements are repeated

chemical change atoms rearrange, physical change molecular structure stays the same

-color

-density

-solubility

-sour taste

-melting point

- flammability

- reacts with acid

-supports combustion

-reacts with water to form gas

-reacts with base

-All matters are made of tiny indivisible particles called "atoms"

- Atoms of same element are similar, atoms of different elements are different

-Elements combine to form compounds, combination of atoms of different element, produce compound atom

-Created by john Dalton

mass is constant (does not change and can not be broken or destroyed) "here to stay"

elements combine in fixed proportion by mass to form compound.

( they also combine in certain ways, never changes)

ALSO, it is fixed because you need to take the whole atom, never can take a portion

example: 1g hydrogen and 8g oxygen and 9g water) FIXED BY MASS

-two elements can form more than one compound

example: hydrogen and carbon

-> one can produce carbon monoxide and another can produce carbon dioxide, etc...

Anode

(reduction because it gains an electron)

"LEO says GER"

Cathode

(Oxidation because it looses an electron)

"LEO says GER"

wihelm Roentgen

J.J thompson with the help of the cathode ray tube ( figured it out when the rays bent)

negative "electron"

"oil drop experiment" which measured the charge of the electron

Henri Bacquerei

(something that is giving energy)

uranium salt

ernest Rutherford

Francis Aston

- gives relative mass of particles

-invented neutron because there was missing mass in the negative/ positive atom

1932

Rutherfrod

this helped discover the nucleus

( the alpha particle hit the middle and bounced all around

hydrogen

potassium

Vanadium

Titanium

Selenium

Krpton

Cobalt

Scandium

Calcium

Chromium

Manganese

Iron

Nickel

Copper

Zinc

Gallium

Germanium

Arsenic

Bromine

Argon

Chlorine

Sulfur

Phosphorus

Silicon

Aluminum

Magnesium

Sodium

Neon

Flourine

Oxygen

Nitrogen

Carbon

Boron

Beryllium

Lithium

Helium

length x length

length x length x length

mass/volume = kg/m^3

distance/ time = m/s

velocity/ time = m/s^2

mass x acceleration= newtons

kg x (m^2/S^2) = joule

energy/ time = watts

force/ area= Pascal

number of protons in the nucleus of an atom

the average mass of all isotopes of an element

atoms of same element with different mass number

mass- atomic number = neutrons

figured out why electrons stay away from the nucleus

leo says ger

is the gain or loosing of electrons

put together the periodic table

organized them into rows (periodic law) and properties of elements

Properties of elements are periodic function of atomic number

R- called period run from top to bottom (But side to side) 1 to 7

C- called groups run from left to right (down if looking for something)

represents elements or main group elements

transitional metals

*Have roman numerals *

Solid, shiny matter, good conductors

- tend to loose electrons (cation)

Liquid, gas, dull, opaque ( not transparent)

-poor conductors

-gain electrons (Anion)

Semi metals

Semi conductors

- Alkai metals (expect hydrogen)

- Alkaine metals (earth metals )

- Boron family

-Carbon family

-nitrogen Family

-Oxygen family

-Halogens

- Noble gases or inhert gases

two or more elements bound together producing a specify structure

Metal with non- metal

- transfer electrons from metal to non- metal

- generally soluble in water

- high melting point

(REMEBER TICS) - TRANSFER IONIC... COVALENT SHARE

- Non-metal and non- metal

- electrons are shared

- low melting point

- low boiling point

Cu copper (II)

use roman numerals

-combine the two elements together

- feCl2

-shows the simplest form of ratio of ions

(answer is 6+)

-because you have to make the whole equation equal zero.

Take the charge at normal state and mult. by how many of the element you have and then subtract or add to get your answer

group 1=+1

group 2=+2

group 3=+3

group 4= -4,+4

group 5=-3

group 6=-2

group 7=-1

group 8=0 they don't loose or gain electrons

(.998(gW/L))(15000mL)(.68gHg)/(1,000,000gW)

It's just grams of mercury per one billion grams of water. You use the density of water to multiply by the volume to find the mass of water, then multiply the ppb to cancel out the grams of water and leave you with grams of HG

CuBr

-molecular compounds

-represented by molecular formula

-DO NOT reduce

Co- carbon monoxide

co2- carbon dioxide

n(2) o(4)- dinitrogen tetraoxide

sF(6)- sulfur hexafluride

- find the mass of each element in the problem

- multiple the mass by how many elements there are

-add up all masses

- divide one elements mass by the total and times by 100

total weight= 249.72 amu

%cu= 25.45

%s=12.84

%o=57.66

%h=4.04

*should equal 100 or 99.99

molecular =c(6) H(8) 0(6) ( not simplified) ( Covalent)

empirical = c(3) h(4) 0(3)( Simplified) ( Ionic)

6.02 x 10^23 = 1 mol

* it is important because every element represents how much atom in a certain element

* this is your conversion factor

Answer= 3.20 x 10^21 x 63.55 / 6.02 x 10^23 = answer (3 sig figs)

answer =6.6165

answer: c1 h2 01

* you might have to multiply if the number is not close to a whole number (2.33) multiply by any number to get actually numbers without decimals

Hydroxide

Cyanide

Nitrate

Phosphite

Sulfate

Permanganate

Chromate

Dichromate

Carbonate

Bicarbonate

Nitrate

Sulfite

Phosphate

Ammonium

Grams/ Molecule or Grams/ formula (weight)

mol x formula ( weight)

*You can no round if the number is 2.33, you must multiply to find a better number

6.02 x 10²³

^{*Arogadro's number}

1. change the percentage

Example= 40.00 to 40.00

2. Divide by it atomic mass

3. Take the answer of all elements and divide by the smelled one

4. The division after step three is your answer

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