Modern Chemistry Chapter 4 Test Vocabulary
photon
Particle of electromagnetic radiation having zero mass and carrying a quantum of energy. Energy is *released* in a _____ when jumping from an excited to a ground state.
waves of quantized energy
Quantum mechanical model explains the atom by treating the electrons as __________
Infra-Red Light
- Longer wavelength, with shorter frequency.
Ultraviolet light
- Shorter wavelength, with higher frequency
orbital
A 3D region around the nucleus that indicates the probable location of an electron. An orbital can hold two electrons with opposite spin
electromagnetic radiation
A form of energy that exhibits wavelike behavior as it travels through space (3.00x10⁸ m/s)
line-emission spectrum
A series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism - The spectrum functions like a DNA fingerprint, it is unique to each element - Can be demonstrated using the Bohr model of a hydrogen atom -produced when an electron moves from a higher energy level to a lower energy level
Pauli exclusion principle
An atomic orbital may describe at most two electrons, each with opposite spin direction. Also no two electrons in the same atom can have the same set of four quantum numbers. ↑↓
noble gas configuration
An outer main energy level occupied, in most cases, by 8 electrons, which is stable
d orbitals or d sublevel
Clover shaped 5 orientations per energy level Total of 10 electrons (2×5) Begins at energy level 3_
electromagnetic spectrum
Combination of all the forms of electromagnetic radiation.
Quantum Theory
Describes mathematically the wave properties of electrons and other very small particles.
wavelength
Distance between corresponding points on adjacent waves. It is measured in meters.
p sublevel
Dumbell shaped 3 orientations per energy level Total of six electrons (2×3) Begins at energy level 2_
Aufbau Principle
Electrons will always occupy the lowest energy level available
photoelectric effect
Emission of electrons from a metal when light shines on a metal.
f orbitals or f sublevel
Has Seven orbitals Has 14 electrons (2×7) Begins at energy level 4_
Magnetic Quantum Number (m)
Indicates the orientation of an orbital around a nucleus (Py, Px, Pz)
ground state
Lowest energy state of an atom. - When an electron moves from a _____ state to an excited state it must *absorb* energy
quantum
Minimum quantity of energy that can be lost or gained by an atom.
18
Number of electrons in the third main energy level, n=3? (2n²)
7
Number of orbitals for the f sublevel?
1
Number of orbitals for the s sublevel?
n²
Number of orbitals per main energy level
frequency
Number of waves that pass a given point in a specific time, usually one second. It is measured in hertz
hertz
One wave per second; 1/s
Hund's rule
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state.
Angular Momentum Quantum Number (ℓ)
Refers to the shape of the suborbitals of an atom. (S, P, D, F) and their availability in each energy level.
Quantum Numbers
Specify the properties of atomic orbitals and the properties of electrons in orbitals.
s sublevel
Spherical Can hold 2 electrons Begins at energy level 1_
excited state
State in which an atom has a higher potential energy than it has in it's ground state. - When an electron moves from an _____ to a ground state, it must release energy, which forms the atomic emmission spectra
Heisenberg Uncertainty Principle
States that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
noble gas
The Group 18 elements (helium, neon, argon, krypton, xenon, and radon)
electron configuration
The arrangement of electrons in an atom
continuous spectrum
The emission of a continuous range of frequencies of electromagnetic radiation. -for the visible spectrum it is the rainbow of colors
Principle Quantum Number (n)
The total amount of energy level an atom has. Energy increases from 1 to 5. It also refers to the average distance of the orbital from the nucleus.
photoelectric effect and the hydrogen line-emission spectrum
The wave model of light does not explain these two phenomena
l = 0, 1, 2
Values of the angular momentum quantum number when n=3?
m = -1, 0, 1
Values of the magnetic quantum number when l = 1?
7.32 x 10¹⁹ Hz
Violet light has a wavelength of 4.10 x 10⁻¹² m. What is its frequency?
Mn
What element has the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵
First find frequency ∨ = c/λ ∨= 3 x 10⁸ m/s ÷ 6.4 x 10⁻⁷ m ∨= 4.69 x 10¹⁴ Hz E = h∨ E= (6.626 x 10⁻³⁴ J.s) (4.69 x 10¹⁴ Hz) E= 3.11 x 10⁻¹⁹ J
What is the energy of a photon of light with a wavelength of 6.4 x 10⁻⁷ m?
2d
Which orbital can never exist according to the quantum description of the atom: 1s 2d 3p 4s 4f 5d 2p
Spin Quantum
Which way it spins. (up or down) (-1/2, + 1/2)
Schrodinger wave equation
describes electrons as waves of specific energies and frequencies helped lay the foundation for the modern quantum theory is an equation that treats electrons in atoms as waves
E=hv
energy equation; The energy of a photon equals Planck's Constant x Frequency J*S. Lower frequencies have lower energies.
sublevel
made up of orbitals s, p, d, f
5
number of d orbitals
3
number of p orbitals
n
number of sublevels per energy level
1s
orbital designation for n=1 l=0
4d
orbital designation for n=4 l=2
c = λν
speed of light = wavelength x frequency As the wavelength decreases the frequency increases, they are inversely proportional.
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹
the electron configuration of K is
2n²
the number of electrons that can occupy an energy level