Test 1 Flashcards
Density =
Mass
——-
Volume
Law of Constant Composition
States that pure compounds always have the same elements in the same mass proportions
Solid
Fixed volume
Fixed shape
Liquid
Fixed volume
No fixed shape
Gas
No fixed volume
No fixed shape
Physical change
The state of matter is not changed
Ex) boiling, mixture
Chemical change
The state of matter changes
Ex) rust, baking
Intensive Physical Properties
Don’t depend on the amount
Ex) BP, density, color
Extensive Physical Properties
Depends on the amount
Ex) mass, volume, energy
Homogeneous mixture
Equally mixed
Heterogeneous mixture
Unequally mixed
C -> K
K = C + 273.15
Precision
The values are close to each other
Accuracy
The mean of the values are close to the target
Significant Figures
*/ least number of sig figs \+- least number of decimal places
Kilo
1000
Hecto
100
Deca
10
Deci
.1
Centi
.01
Milli
.001
Micro
.000001
Proton
+ charge
Atomic number
of protons
Neurons
Neutral charge (Mass # - Atomic #)
Isotope
Atoms with same atomic number (protons) and a different mass number (neutrons)
Mass number
Protons and neutrons
Transition Metal
Middle group
Inner Transition Metal
Lower group
Main-Group Elements
Everything but middle and bottom
Alkaline Metal
Group 1
Alkaline Earth Metals
Group 2
Halogens
Group 7
Noble Gas
Group 8
Covalent Bonding
2 non metals
Sharing of electron pairs
Ionic Bonding
Metal and non-metal
Attraction of oppositely charged ions
Rutherford’s gold foil experiment
Alpha particles hit a gold foil sheet. Most particles weren’t scattered but some were at large angles!
ATOM HAS A SMALL AND DENSE NUCLEUS.
Millikan oil drop experiment
Balanced the gravitational force of the negatively charged oil droplets. He determined the charge of electrons was a discrete value.
MASS TO CHARGE RATIO.
JJ Thompson
Discovered cathode rays and the negatively charged electron and that atoms were not indivisible.
PLUM PUDDING MODEL
Dalton’s Atomic Theory
Matter composed of indivisible atoms. (Proved wrong by JJ Thompson)
Elements are composed of 1 type of atom.
Compounds are composed of 2 or more elements in fixed proportions.
Chemical reactions involve the rearrangement of atoms in reacting substance.
Law of Multiple Proportions
When two elements combine to form more than one compound it is in the ratio of whole numbers.
Plum pudding model
JJ Thompson electrons spread around an atom.
Nuclear model
Rutherford electrons with small dense nucleus
Chapter 6 Equations
E_n = -R_H
——-
n^2
V ¥ = c
E = h v
E = h c
——
¥Electromagnetic Radiation Properties
Wave-like
Particle-like
EMR wave-like properties
Wavelength ¥
Frequency v
Wavelength
¥ distance between each point in a cycle of the wave (m)
Frequency
V number of wavelengths that pass a point in a given time (s^-1 Hz)
Speed of Light
C = 3.00 * 10^8 m/s
Radio
Lower energy
Lower frequency
Higher wavelength
Gamma
Higher frequency
Higher energy
Lower wavelength
Planck’s constant
h= 6.63*10^-34 Js
E = nhv
Vibrations have discrete energies
Photoelectric effect
The ejection of electrons from the surface of metal by light.
Rays
Gamma-xray-ultraviolent
Visible (purple, blue, green, yellow, red)
Infared-microwave-radio
Rhydberg
R_H = 2.18*10^-18 J
Bohr model
Small positively charged nucleus surrounded by electron shells orbiting the nucleus
Absorption
Ground state to excited state
Emission
Excited state to ground state
De Broglie
Matter can exhibit wavelike properties
¥= h
—
mv
n
Principle quantum number
n= 1,2,3…
Determines the energy of electron
l
Angular momentum quantum number
l = n-1
Determines the shape
m_l
Magnetic quantum number
m_l = -l to +l
Determines orientation of orbital
m_s
Spin quantum number
m_s = +/- 1/2
Determines the spin
Paramagnetic
Unpaired electron
Diamagnetic
Paired electrons
Pauli exclusion principle
No 2 electrons can be the same
Building up principle
Orbitals are filled in order
Spd
Hunds rule
Fill each subshell first before putting in opposite spin
Uncertainty principle
The momentum and position cannot be determined at the same time
Exceptions to Building up
D4 d9 f6 f13
