Chemistry Midterm Review

This includes... - Atomic Theory - Development and Trends of the Periodic Table - Electrons & the Atom - Radioactive Decay, Nuclear Reactions, & their Effects - Light and Quantized Energy

protons

1 of 3 subatomic particles a positive electric charge in the atom's nucleus with an atomic mass of 1 amu

neutrons

1 of 3 subatomic particles a 'neutral charge' that does not actually have an electric charge

it is found in the nucleus of an atom with an atomic mass of 1 amu

electrons

1 of 3 subatomic particles a negative electric charge that orbits around the nucleus, with an atomic mass of 1/1836 amu

forms chemical bonds and determines the chemical properties of an atom

Law of Conservation of Mass

a part of dalton's atomic theory states that within a chemical reaction, matter is never created or destroyed, and can only be converted

Law of Definite Proportions

a part of dalton's atomic theory elements in a compound will always be combined in a specific ratio

Law of Multiple Proportions

a part of dalton's atomic theory elements that make up compounds will always be in the whole numbers

Indivisible

all atoms are indivisible and is the smallest unit of matter

Identical

all elements that are the same have the same mass and properties, and differing elements have different mass and properties

Thomson

discovered the different charges within an atom, but did not name them

Rutherford

states that protons and neutrons are in the center of the nucleus and electrons surround the nucleus, found atoms are mostly empty space

Quarks

an elementary particle makes up of protons and neutrons and has different 'flavors'

up, down, strange, charm, bottom, top

Leptons

an elementary particle makes up electrons, and has two types: muon and tau

Grand Unified Theory

originally believed to be all one force, but states that there are the fundamental forces of the Standard Model: electromagnetism, weak nuclear force (nuclear decay), and strong nuclear force (binding protons and neutrons)

atomic number

the number of protons in an atom

groups

families in a series of vertical columns

group 1 - Alkali Metals group 2 - Alkali Earth Metals group 3-12 - Transition Metals groups 17 - Halogens group 18 - Noble Gases

periods

series of rows of horizontal element groups

elemental series 57-71 - Lanthanides elemental series 89-103 - Actinides

noble gasses

naturally occurring gasses of group 18 that have NO electronegativity

Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn), Oganesson (Og)

atomic radius

half the distance between adjacent nuclei in a crystal of an element

ion

a atom or group of atoms that have a positive and negative charge

a charged particle

anion

a negative ion that has more electrons than protons

cation

a positive ion that has more protons than electrons

ionization energy

the energy required to remove an electron from a gaseous atom

electronegativity

an element indicates the relative ability of its atoms to attract electrons in a chemical bond

valence electrons

electrons in an atoms outermost energy level that determines an elements chemical properties

can cause instability

electron configuration

determines the chemical properties of an element

can be determined by position on the periodic table

s block

comprised of alkali metals and alkali earth metals

d block

transition metals

p block

nonmetals and metalloids

f block

lanthanides and actinides

radioactivity

the process by which some substances emits or spontaneously radiates energy

band of stability

having too many neurons to be stable

those below band of stability have too many protons

positron emission

a type of radioactive decay called beta decay

the nucleus converts to a neutron by releasing a positron

positron

made by protons, but 2000x smaller has all properties of an electron apart from their polarity

it is an electron with a positive electric charge

radioactive decay series

a series of nuclear reactions that begin with an unstable nucleus and results with the formation of a stable nucleus

half life

the required amount of time for 1/2 of a radioisotope nuclei to decay into half of its mass

a loss of radioactivity

forms of radioactive decay

beta decay, alpha decay, and positron emission

transmutation

the conversion of 1 chemical element or isotope into another chemical element

when the number of protons or neutrons change

alchamy

a form of transmutation

nucleon

a proton or neutron

radiochemical dating

typically to determine time periods relating to its formations, it dates materials where radioactive impurities are selectively incorporated when they are formed

mass number

aka isotope number the number after an elements name that represents the sum of protons and neutrons

induced transmutations

aka nuclear fusion or nuclear bombardments the process of striking a nuclei with high velocity particles

hydrogen isotopes

decterium (H^2) and tritium (H^3

light nuclei

gain stability by undergoing nuclear fusion

heavy nuclei

gain stability by undergoing nuclear fission

nuclear fission

the splitting of a nucleus into fragments

highly difficult and requires a mass amount of energy

nuclear fusion

the combining of a nucleus to produce heavy elements and a mass amount of energy

due to hydrogen isotopes and helium

transuranium element

elements with an atomic number larger than 92

critical mass

the smallest amount of fissile to sustain a nuclear chain reaction

mass defect

the mass of the energy is the sum of the constituent particle

the difference is the mass of particles

thermonuclear reaction

any reaction between two different atomic nuclei and subatomic particles

breeder reactors

a nuclear reactor that generates energy to feed or kickstart nuclear reactors

produces toxic energy in masses that can lead to nuclear meltdowns/chemical failure

cold fusion

only a theory, has NOT been produced 'safe' fusion that makes no waste

ionizing radiation

radiation energy that has enough energy to ionize any matter it comes in contact with

Geiger counter

ionization radiation detection device

electromagnetic radiation

a form of energy that exhibits wavelike behavior as it travels through space

wavelength

based on x-axis the distance over which the wave's shape repeats

the length from crest to troph

crest - top troph - bottom

frequency

the number of occurrences of a repeating event per unit of time, measured in hertz (Hz)

amplitude

based on y-axis the maximum magnitude of displacement, measured in meters (m)

electromagnetic spectrum

the spectrum of electromagnetic radiation that ranges based on wavelength and photon energies

all forms of electromagnetic radiation

atomic emission spectrum

the set of frequencies of the electromagnetic waves emitted by atoms of an element

causes emission of colors

quantum

the minimum amount of a physical entity involved in an interaction

photoelectric effect

the emission of electron radiation when energy hits a material, ie light and mirrors

Plank's constant

a number that defines the amount of energy in quanta and expresses how small things can be in quantum mechanics 6.23 x 10^-34 J/s (joules/second)

photon

an elementary particle that is a quantum of the electromagnetic field, includes radiation like light and radiowaves

quantum number

an assigned number to each orbit

quantum mechanical model

electrons are treated as wave forms

how electrons travel along a path

ground state

lowest state of energy in an atom or another particle

atomic orbital

a functioning description of the location and behavior of an electron surrounding nucleus

principal quantum number

the energy of an electron and the most probable distance of an electron from the nucleus

principal energy level

the shell or orbital in the electron is located relative to the nucleus

de Brogile equation

allows for the calculation of the wavelength of any moving object

A - wavelength v - velocity n - plank's constant m - mass

Heisenburg uncertainty principle

states it is impossible to accurately determine both momentum and positron of an electron in high precision

emphasizes the unpredictability of principal

electron configuration

the arrangement of electrons in an atom, usually represented with orbital diagrams or configuration notation

ground state electron configuration

the most stable, lowest energy arrangements of electrons

aufbau's principle

to build up or arrange the ground state of an atom, filling the lowest energy level, then filling the highest available energy level

Pauli exclusion principal

states that no 2 electrons in the same atom have identical values for all 4 of their quantum numbers

Hund's rule

exclusive to d-block states that every orbital is singly occupied with one electron before any other orbital is double occupied, and all occupants must have same spin

electron dot structure

a representation of the valence electrons of an atom that uses dots around the symbol of the element

reaction rate

the charge in concentration of a reactor/product per unit of time calculated in moles per liter per second (mol/L/s)

Le Chatlier's Principal

states if stress is applied to a system at equilibrium, the system shifts in the direction that relieves stress

stress upsets equilibrium, add product - shift to left remove product - shift to left

free energy

the energy that is available to do work, the difference in change of enthalpy and the product of the enthalpy change and absolute temperatures

chemical equilibrium

a state in which the forward and reverse reactions balance each other because they take place at equal rates

reversible reaction

a reaction in which the conversion of reactants occur simultaneously

law of chemical equilibrium

in a chemical system, the concentration of products and concentration of reactants are at equilibrium

equilibrium's constant

the ratio between the amount of reactant and the amount of product used to determine chemical behavior

homogeneous equilibrium

all species in the reaction are present in the same phase

heterogeneous equilibrium

all species in the reaction are present in more than 1 phase

solubility

the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure

solubility product constant

the equilibrium constant for a solid substance dissolving in an aqueous solution

due to common ion effect

common ion

an ion that is common to 2 or more ionic compounds

common ion effect

lowering the solubility of a substance because of the presence of a common ion