Atoms

Density is the XXX of XXX in a substance or mixture

• Higher density = more XXX in a given XXXX

If density is greater than water or 1, it will XXX. 

If density is less than 1, it will XXX. 

XXX/XXX=denisty XXX/XXX=d  1mL=XXX

Density is the concentration of mass in a substance or mixture

• Higher density = more mass in a given volume

If density is greater than water or 1, it will sink. 

If density is less than 1, it will float. 

Mass/Volume=denisty g/mL=d  1mL=1cm^3/cc 

Fahrenheit: symbol-X; melting point/freezing point of water: X F; Boiling/Condensation of water: X F

Celsius: symbol-X; melting point/freezing point of water: X C; Boiling/Condensation of water: XX C

Kelvin: symbol-X; melting point/freezing point of water: XXX C; Boiling/Condensation of water: XXX C

- If you want to get kelvin from fahrenheit you need to turn it to XXX first. 

- Celsius and kelvin are XXX XXX

Fahrenheit : symbol-F; melting point/freezing point of water: 32 F; Boiling/Condensation of water: 212 F

Celsius: symbol-C; melting point/freezing point of water: 0 C; Boiling/Condensation of water: 100 C

Kelvin: symbol-K; melting point/freezing point of water: 273 C; Boiling/Condensation of water: 373 C

- If you want to get kelvin from fahrenheit you need to turn it to celsius first. 

- Celsius and kelvin are directly proportional

Atoms are composed of three types of subatomic particles: XXX, XXX, and XXX. 

Subatomic particle: Proton. Symbol: X  Location: X. Relative charge: X. Relative mass: X

Subatomic particle: Neutron. Symbol: X Location: X Relative charge: X Relative mass: X 

Subatomic particle: Electron. Symbol: X Location: X. Relative charge: X Relative mass: X

The electron stays in the atom and floats around the nucleus because of the….

Atoms are composed of three types of subatomic particles: Protons, electrons, and neutrons. 

Subatomic particle: Proton. Symbol: P/+ Location: In nucleus. Relative charge: +1. Relative mass: 1 

Subatomic particle: Neutron. Symbol: N Location: In nucleus. Relative charge: 0 Relative mass: 1 

Subatomic particle: Electron. Symbol: e- Location: Around nucleus. Relative charge: -1. Relative mass: 0. 

- The electron stays in the atom and floats around the nucleus because of the positive charge from the protons, charges attracts. 

Atomic #: XXX number on periodic table. XXX number on atomic notation. Includes number of XXX. XXX changes for an element even in different XXX. The XXX is the identifier of an atom, always the XXX. 

# of electrons: all the elements on the periodic table are XXX so same as the XXX number, if no charge is associated with it. 

Atomic mass #: XXX number in periodic table. XXX number in aonimc notation, always XXX this number to a whole number in XXX XXX. 

You find neutron amount by subtracting the XXX XXX XXX to the XXX number. 

- Also, you can write the isotope name as follows: Oxygen-16 (16 being the different XXX XXX XXX).

Atomic #: Top number on periodic table. Button number on atomic notation. Includes number of protons. Never changes for an element even in different isotopes. The proton is the identifier of an aton, always the same. 

# of electrons: all the elements on the periodic table are neutral so same as the proton number, if no charge is associated with it. 

Atomic mass #: bottom number in periodic table. Top number in aonimc notation, always round this number to a whole number in atomic notation. 

You find neutron amount by substrating the atomic mass number to the proton number. 

- Also you can write the isotope name as follows: Oxygen-16 (16 being the different atomic mass # not the atomic number). 

Relative charge is calculated by: XXX number minus XXX number

- Isotopes are atoms of the XXX element that have the same number of XXX but different XXX or different number of XXX. Same XXX/XXX; different XXXX/XXX

- Atomic mass average is weighed like this: (XXX given XXXX %/ XXX) +  (XXX given XXX %/ XXX)+ ETC. If the abundance was not given for one of them subtract that abundance percentage until you are able to get XXX%.

Relative charge is calculated by: Proton number minus electron number

- Isotopes are atoms of the same element that have the same number of protons but different masses or different number of neutrons. Same protons/atomic number; different atomic mass/neutrons. 

- Atomic mass average is weighed like this: (mass given abundance %/ 100) +  (mass given abundance %/ 100)+ ETC. If the abundance was not given for one of them subtract that abundance percentage until you are able to get 100%.

Atomic mass is the XXX XXX mass of all the naturally occurring XXX of an element, measured in atomic mass units (XXX).

It takes into account both: The XXX of each XXX; The XXX XXX (how XXX each XXX is in XXX)
Where is Atomic Mass Found on the Periodic Table?

Atomic mass is usually the XXX number shown XXX the element symbol.

	Atomic Mass	Mass Number
What it is	XXX XXX of all XXXX	Total number of XXX + XXX
Decimal or whole?	XXXX	XXX
Found on	XXX	XXX
Varies between atoms?	XXX — XXX for element on XXX XXX	XXX — depends on the XXX

Atomic mass is the weighted average mass of all the naturally occurring isotopes of an element, measured in atomic mass units (amu).

It takes into account both: The mass of each isotope; The relative abundance (how common each isotope is in nature)
Where is Atomic Mass Found on the Periodic Table?

Atomic mass is usually the decimal number shown below the element symbol.

	Atomic Mass	Mass Number
What it is	Average mass of all isotopes	Total number of protons + neutrons
Decimal or whole?	Usually a decimal (e.g., 35.45)	Always a whole number (e.g., 35 or 37)
Found on	Periodic Table	Not on the periodic table (must be given)
Varies between atoms?	No — same for element on periodic table	Yes — depends on the isotope

John Dalton proposed the following on the atom in 1803. Disproven?

— All atoms of an element are XXX and have the same XXXX.

— Atoms of different XXX combine to form XXXX

— An element is composed of XXX, XXX, XXX particles called XXX.

— Compounds contain atoms in small whole number XXX.

— Atoms can combine in XXX than XXX XXX to form different XXXX.

John Dalton proposed the following model of the atom in 1803. The first two have been disproven.

1. An element is composed of tiny, indivisible, indestructible particles called atoms. XXXX

2. All atoms of an element are identical and have the same properties. XXXXX

3. Atoms of different elements combine to form compounds

4. Compounds contain atoms in small whole number ratios: H2O for water is always H2O in that 2:1 ratio. H4O2 is the same as H2O but you musy simplify. 

5. Atoms can combine in more than one ratio to form different compounds.