Chemistry Final Exam
Terms
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- Thomson
- Cathode ray tubes --> electrons are attracted to + pole of plate, deflected by a magnet
- Millikan
- oil drop experiment --> electron has negative charge, mass is 1/2000 mass of H atom
- Rutherford
- alpha particles --> tiny amount of space with dense. + charged matter (Nucleus)
- Chadwick
- discovered neutron
- Bohr
- Bohr model of atom, orbitals, lowest energy states, energy from orbit changes
- Lavoisier
- conservation of matter
- Proust
- Definite mass percentages
- Dalton 1
- all matter is composed of atoms
- Dalton 2
- atoms are indivisible and indestructible
- Dalton 3
- Atom's mass distinguishes one atom from another
- Dalton 4
- Atoms combine in Definite Whole # Ratios when forming compounds
- Law of Conservation of Mass
- mass is neither destroyed nor created during ordinary chemical or physical reactions
- Law of Definite Proportions
- a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size or source of the compound
- Law of Multiple Proportions
- if 2+ diff. compounds are composed of the same 2 elements, then the ratio of the masses of the 2nd element combined with a certain mass of the 1st element is always a ratio of small whole proportions
- Electromagnetic Radiation
- a form of energy that exhibits wave-like behavior as it travels through space
- Types of electromagnetic radiation
- visible light, x-rays, UV light, infrared light, microwaves, radio waves
- Speed of light
- 3.0*10^8 m/s
- Wavelength
- distance between crests on adjacent waves (m,cm,nm)
- Frequency
- # of waves that pass a given point in a specific time
- ratio of wavelength to frequency
- Speed of light (c) = wavelength*frequency
- Planck's constant
- 6.626810^-34
- Energy of a photon equation
-
E-photon = Planck's constant*frequency
(E = hv) - Quantum
- the minimum quantity of energy that can be lost or gained by an atom
- H-Atom Line-Emission Spectrum
- a series of specific wavelengths from when the visible portion of the emitted light is passed through a prism
- Equation for the emission of energy
- Ephoton= excited - ground
- photoelectric effect
- the emission of electrons from a metal when light shines on it, a minimum frequency of light required
- UV light
- Lyman series, longer transitions
- Red Light
- Balmer series, medium transitions
- Visible Light
- Paschen series, shorter transitions
- Light behaves as a wave in the
- Photoelectric effect and the line emission spectrum
- Light behaves as a particle when
- Quantum numbers and the Bohr's model of the atom
- Debroglie's equation
- wavelength = planck's constant/(mass*velocity)
- Quantum Mechanics theory was deriven by
- Shrodinger
- Quantum Mechanics theory parts
-
Wave Functions
Energy Levels
Principal Quantum Numbers - Principal Quantum Numbers (n)
-
describe main principal energy levels/states
n = 1,2,3... - n^2 represents
- # possible orbitals
- 2n^2 represents
- maximum # electrons
- Angular Momentum QN (l)
- type of orbital/orbital shape
- Principal QN rule
- n = 1,2,3...
- Angular Momentum QN rule
- l < n-1
- angular momentum value for s orbital
- 0
- Magnetic QN meaning
- orientation of an orbital in space
- Magnetic QN rule(ml)
- -L<0<L
- Pauley Exclusion Principle
- no 2 electrons in the same atom can have the same 4 QNs
- Spin QN
- +1/2 or -1/2
- Aufbau Principle
- electrons go into the lowest energy orbitals
- Hund's rule
- electrons occupy equal energy orbitals singly with parallel spin
- Mendeleev organized periodic table according to?
- atomic mass
- Moseley organized the periodic table according to?
- atomic #
- Group 1
- Alkali metals
- Group 2
- Alkaline-Earth Metals
- Group 17
- Halogens
- Group 18
- Noble Gases
- 2 columns at bottom of periodic table are called?
- Lactanides and Actinides
- Atomic Radius horizontal pattern?
- decreasing
- Why do the atomic radii __________ horizontally?
- Increasing positive charge of nucleus, pulled closer to more protons
- Atomic Radius vertical pattern?
- increasing
- Why does the atomic radius _________ vertically?
- electrons filling successively higher main energy levels located farther from the nucleus
- Ionization Energy is...
- the energy required to remove one electron from a neutral atom of an element
- Ionization Energy horizontal pattern?
- Increasing
- reason for Ionization energy horizontal energy pattern
- increasing nuclear charge which more strongly attracts electrons in the same energy level, more difficult to remove
- Ionization energy vertical pattern?
- decreases
- Reason for vertical ionization energy pattern
- removed more easily because they are further from the nucleus
- Electron affinity is...?
- the energy change that occurs when an electron is acquired by a neutral atom
- Electron affinity horizontal pattern?
- Increasing (negatively)
- Electron affinity vertical pattern?
- decreases (negatively)
- Cation
- a positive ion
- Cationic radii and ionic radii ___ across a period?
- decrease
- Why do Cationic radii and Anionic ___ across a period?
- because electron cloud shrinks, protons have more affect
- Cationic radii and Anionic ___ down a group?
- increase
- Why do ionic radii ___ down a group?
- because outer electrons are in higher energy levels
- Anion
- a negative ion
- Electronnegativity is...?
- A measure of the ability of an atom in a chemical compound to attract electrons
- The most electronegative element is ?
- Fluorine
- Electronnegativity ____ across a period
- increases
- Why does electronnegativity ___ across a period?
- Closer to noble gas configuration
- Electronegativity ____ down a group
- decreases (in general)