Chemistry Chapter 4 Flashcards
According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels?
electrons
The line emission spectrum is caused by the energies released when electrons…….
jump from higher energy level to a lower energy level
Because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen
releases energy of only certain values
Which color of light in the visible spectrum has the longest wavelength?
red
A quantum of energy is the …..
minimum quantity of energy that can be lost or gained by an atom
Bohr’s model correctly explains the spectra of atoms with how many electrons?
one
A form of energy that exhibits wave behavior as it travels through space is…?
microwave radiation
infrared radiation
ultraviolet radiation
In the equations λν = c, c represents ?
the speed of light
The process of an atom releasing energy when it moves to a lower energy state is called
emission
In the Bohr model of the atom, in which orbit is an electron in its lowest energy state?
in the orbit closest to the nucleus
The common characteristics shown by X-rays, visible light, infrared radiation, and radio waves is that they all have the same….
speed
A quantum of electromagnetic energy is called a …
photon
An optical instrument that separates light entering it into component wavelength is a …
spectrascope
The lowest total energy of the electron in a hydrogen atom occurs when the electron is in the state called…
ground state
What happens to frequency when wavelength increases
decreases
What happens to frequency when energy increases?
increases
How does Bohr’s model of the atom differ from Rutherford’s
Bohr’s model shows the different levels and is more detailed, which Rutherford’s is a vague outline of what the cell looks like and where the electrons are
Exclusion principle
Pauli
wave-particle duality
de Broglie
Wave equation
Schrodinger
uncertainty principle
Heisenberg
Number of energy levels and describes electron cloud size
n-energy
Shape of electron cloud
l-shape
direction in space of each orbital
m-orientation
spin of the electron
s-spin
If n=4, there may be… sublevels
16 in total
4 in types
The p sublevel may contain… pairs of electrons or orbitals
3
Two electrons occupying the same orbital must have opposite…
spins
The last electron in an oxygen atom enters the … orbital
2p
How many sublevels are possible for each of the following
n=1
n=3
n=6
1
3
6/4
How many orbitals are there in the following sublevels.
p
d
f
3
5
7
The size and shape of an electron cloud are most closely related to the electron’s
energy
The quantum number that indicates the position of an orbital about the three axes is space is the
magnetic quantum number
An orbital that would never exist in the quantum description of atom is
2d
For n=2, the number of possible orbital shapes is
4
The number of particles found in the nucleus of an atom
mass number
The method of studying substances that are exposed to continuous exciting radiation is called…
spectroscopy
a negative electrode
anode
atoms possessing the same number of protons but different number of neutrons
isotopes
the number of cycles or peaks of a wave that occur in a unit of time
frequency
A unique set of wavelengths absorbed by a particular substance
spectrum
The smallest and least energetic path of an electron around a nucleus
ground state
A particle found in the nucleus
nucleon
A negative particle having 1/1836 the mass of a proton
ellectron
The average mass of an element
atomic mass
1/12 the mass of the carbon-12 isotope
Atomic mass unit
a positive electrode
cathode
a quantum of radiant energy
photon
the emission of electrons from the surface of a metal when struck by light
photoelectric effect
the number of protons in an atom
atomic number
the unit of frequency
herts
the particles which make up atoms are called
subatomic particles
the physical distance between the peaks of a wave
wavelength
energy that exhibits wavelike behavior as it travels through space
electromagnetic spectrum
emission of electrons from a metal when light shines on the metal
photoelectric effect
states that the energy was emittited in small, specific amounts of energy
Max Planck
Minimum quantity of energy that can be lost or gained by an atom
quantum
theory for a quantum
E=hv
particle carrying a quantum energy and having zero mass
photon
atoms absorb energy from heat or electricity and give off the energy as light
bright line spectrum
___ explains the bright line spectra
Bohr’s model
an electron goes to _____ state, then ___ then goes to a ____ level and becomes____ and returns to a _____, ___ is released as photon_spectral lines
ground excited higher unstable lower energy
electrons have wavelength properties
de Broglie
it’s impossible to determine simultaneously the position and velocity of an electron
uncertainty Principle’
Heinsenberg
Dual wave particle properties
Schrodinger Wave equation
describes mathematically the wave properties of electron
quantum theory
average region of the most probably electron location
orbital
energy level(1-7)
principle quantum number
shape of orbital= s p d f
1 3 5 7
orientation of the orbital around the nucleus
magnetic quantum number
indicates the 2 fundamental spin states of an electron in an orbital
spin quantum number
how many electrons can an orbital carry
and what must they have
2
opposite spins
no 2 electrons have the same 4 quantum numbers
Pauli’s Exclusion Principle
an electron occupies the lowest energy orbital that can recieve
Aufbau Principle
A 2nd electron is not added to an orbital until each orbital in the sublevel contains one
Hund’s rule
what’s the maximum # of electrons in the outer level of an atom
8