Chemistry (H) Chapter 4 Study

H

Hydrogen

Li

Lithium

Na

Sodium

K

Potassium

Rb

Rubidium

Cs

Cesium

Fr

Francium

Be

Beryllium

Mg

Magnesium

Ca

Calcium

Sr

Strontium

Ba

Barium

Ra

Radium

B

Boron

Al

Aluminum

Ga

Gallium

C

Carbon

Si

Silicon

Ge

Germanium

Sn

Tin

Pb

Lead

N

Nitrogen

P

Phosphorus

As

Arsenic

Sb

Antimony

Bi

Bismuth

O

Oxygen

S

Sulfur

Se

Selenium

Te

Tellurium

Po

Polonium

F

Fluorine

Cl

Chlorine

Br

Bromine

I

Iodine

At

Astatine

He

Helium

Ne

Neon

Ar

Argon

Kr

Krypton

Xe

Xenon

Rn

Radon

Ac

Actinium

La

Lanthanum

U

Uranium

Pu

Plutonium

who discovered the solid atom in which year?

john dalton in 1803

what did John Dalton believe the solid atom was?

solid, indivisible atom. he was shattered by the discovery of subatomic particles

who discovered the plum pudding atom in which year?

J.J. thomson in 1898

what was the plum pudding atom

a sphere of positive protons in which negative electrons are embedded throughout

what were two things that J.J. Thomson couldn’t explain about the plum pudding atom

the arrangement of the protons, and the ease with which electrons were moved between atoms to form ions

who discovered the nuclear atom in which year?

ernest rutherford in 1911

what was the nuclear atom

a tiny, dense, positive nucleus surrounded by a large volume of empty space that contained electrons

what could Ernest Rutherford not explain about the nuclear atom

he couldn’t explain why the positive nucleus did not attract the negative electrons around the atom

who discovered the planetary atom in which year?

niels bohr in 1913

what was the planetary atom?

electrons orbiting the nucleus in “allowed energies” like planets orbiting the sun

what did Niels bohr say about the planetary atom?

electrons can only exist in the atom if they have certain “allowed energies'“ (energy level)

definition of energy level

a region around the nucleus in which electrons of a certain energy may exist

electrons may only exist ____ energy levels, never ____ energy levels

INSIDE, BETWEEN

ground state meaning

electrons are normally in the lowest available energy level

excited state meaning

electrons can absorb energy to temporarily go into a higher energy level

orbit meaning

a fixed path around the nucleus that contains electrons of a certain energy

light definition

a form of electromagnetic radiation (energy waves) visible to the human eye

wavelength definitio, another name for it. uses which units?

distance between 2 crests, lambda. meters

frequency definition

number of waves that pass a point per unit of time

what are the two symbols for frequency

Hz, or s^-1

frequency equation

frequency = (speed of light) / (wavelength)

what is the constant speed of light

2.998 × 10^8 m/s

continuous spectrum

having no breaks/gaps throughout wavelength range (ROY G BIV)

bright line spectrum

characteristic set of spectral lines given off by an excited atom

what is another name for the bright line spectrum?

atomic emission spectrum

who made the quantum theory in which year?

max planck in 1900

what is max planck’s Quantum Theory

light travels in tiny packets of energy in a fixed size called QUANTA or photons

what is planck’s constant?

6.6262 × 10^-34 Js

what is the energy of a photon equation in Quantum Theory

E= hv

what is E in E=hv

energy of a photon in Joules

what is h in E=hv

planck’s constant

what is v in E=hv

the frequency of the light

each line on a bright line spectrum corresponds to a _______ between two energy levels

specific jump

one problem with the Bohr atom

the atom only worked with hydrogen like atoms and ions (atoms with 1 electron)

what did louis de broglie predict in 1924?

all matter exhibits wavelike motions

what is classical mechanics?

describes motion of objects larger than atoms

what is quantum mechanics

describes motion of subatomic particles and atoms as waves that lose energy as quanta

who discovered the electron cloud atom in which year?

erwin schrödinger in 1926

how did bohr and schrödinger agreed in the description of the atom

all atoms have a nucleus and electrons move around the nucleus within energy levels

how did bohr describe the atom in his own words?

described that electrons follow nice neat paths called ORBITS

how did schrödinger describe the atom in his words?

electrons orbit the nucleus in mathematically probability regions called orbitals, which is the electron cloud atom

wave equation definition

mathematical description of the wavelike properties of electrons

equation to find amount of electrons in a certain energy level

2n² (n=energy level)

energy levels (shells) are divided into ______

sublevels (subshells)

how many orbitals and maximum amount electrons are in the sublevel “s

1 orbital, 2 electrons

how many orbitals and maximum amount electrons are in the sublevel “p”

3 orbitals, 6 electrons

how many orbitals and maximum amount electrons are in the sublevel “d”

5 orbitals, 10 electrons

how many orbitals and maximum amount electrons are in the sublevel “f”

7 orbitals, 14 electrons

how many electrons are there per orbital?

2 electrons

aufbau principle

electron configurations build up upon the proceeding elements

degenerate orbitals

orbitals with the same energy, orbitals in the same sublevel

which sublevels are degenerate orbitals important for?

sublevels p, d, f, NOT s

hund’s rule

when filling degenerate orbitals, each orbital gets one electron with the same spin before any orbital gets its second electron with the opposite spin

which shell is always at the highest energy level?

valence shell