Exam 4 Flashcards by Emily Klatzer

Excited atom makes what

Light emitted

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Atom plus light absorption makes what

Excited atom

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Distance between adjacent peaks on the wave (m)

Wavelength (λ)

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Number of waves that pass a point per second (Hz or 1/s)

Frequency (v)

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Vertical distance from the mid-line to the peak

Amplitude (intensity)

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Speed of light (c)

3.00 * 10^8 m/s (in a vacuum)

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Wavelength & frequency have what relationship

Inverse

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Who developed a theory for light, proposing that light waves consists of 2 components; a vibrating electric field & a vibrating magnetic field

Maxwell

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Who studied radiation emitted by matter & postulated that energy in matter is quantized

Max Planck

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Smallest increment of energy that can be emitted or absorbed in the form of electromagnetic radiation

Quantum of energy

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Energy equation of a single quantum

E=hv (E-energy J, v-frequency 1/2, h-Planck’s constant)

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Plancks constant

6.6310^-34 Js

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Light can cause electrons to be ejected from a metal surface

Photoelectric effect

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If light has a frequency less than the threshold frequency, what happens

No electrons ejected

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If light has a frequency greater than the threshold frequency, what happens

Number of electrons ejected is proportional to the light intensity

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Who considered that light is composed of a stream of particles (photons- quantum packets of energy), extended Planck’s ideas

Albert Einstein

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Electromagnetic radiation has what properties

Wave-like & particle-like properties

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E=hv can also be written as

E=hc/λ

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Short wavelengths have high energy and are

Damaging to life, like X rays

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Long wavelengths have low energy and are

Safe, like radio waves

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Atom that has the simplest atomic spectrum

Hydrogen atom

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Each atom has its own unique

Atomic spectrum

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Who studied the lines in the visible portion of the hydrogen spectrum (400-700nm)

JJ Balmer

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Rydberg equation for calculating the emission lines in the hydrogen spectrum

1/λ=Rh[(1/n^2i) - (1/n^2f)]

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Rydberg's constant

109,678cm^-1

nf=1; ni=2,3,4... (ultraviolet)

Lyman series

nf=2; ni=3,4,5...(visible)

Balmer series

nf=3; ni=4,5,6...(infrared)

Paschen series

nf=4; ni=5,6,7... (infrared)

Brackett series

Danish physicist who developed a theoretical model for the hydrogen atom that restriceted on the sizes of the orbits & the energy that the electron can have in a given orbit

Niels Bohr

In Bohr's model, lowest energy atoms are what

n=1, E<0

In Bohr's model, highest energy atoms are what

n=∞, E=0

Electron in ground state absorbs energy & does what

Moves to a higher energy orbit, excited state

Photon emitted, meaning what

ni>nf, ΔE is -

Photon absorbed, meaning what

Hypothesis that suggested that if electromagnetic radiation can have particle-like properties, then electrons may also possess wave-like properties

de Broglie's hypothesis

Combining Einstein's theory with de Broglie's hypothesis, you get what equation

λ=h/mc (mc is momentum- mass * velocity)

Two waves add together when waves have the same frequency & are in phase with each other

Constructive interference

Two waves with same frequency but are out of phase

Destructive interference

Who applies wave properties of matter to explain atomic properties, created wave mechanics

Erwin Schrodinger

Electrons exist only where what

Waves reinforce each otherq

An atomic orbital is characterized by what

Energy, size, shape, orientation in space

s orbitals have what shape

Spherical

p orbitals have what shape

Two lobes about the nucleus

p orbitals shape

Balloons on each side of nucleus, vary in orientation

d orbitals shape

Complex, four lobes of electron density, differ in orientation

f orbitals shape

Very complex, 8 lobes of electrons about nucleus

Quantum number that determines the energy & size of an orbital

Principal quantum # (n=1,2,3... ∞)

Quantum number that determines the shape of the orbital

Angular momentum quantum # (l=0,1,2,3...n-1)

l=0

l=1

l=2

l=3

l=4

l=5

Quantum number that describes the orientation in space relative to other orbitals in that same subshell

Magnetic quantum # (ml= -l, -l+1,....+l)

s orbitals have a spherical shape

n=1 to ∞, l=0, ml=0

p orbitals have the same shape, size, & energy- differ only in orientation in space, consist of two lobes of electron density about the nucleus

n≥2, l=1, ml=-1,0,1.

d orbitals have 5 individual orbitals, complex shape, differ only in orientation in space

n≥3, l=2, ml=-2, -1,0,1,2

f orbitals have 7 individual orbitals, complex shape consisting of 8 lobes of electron density, differ only in orientation in space

n≥4, l=3, ml=-3,-2,-1,0,1,2,3

Quantum number describing an electrons spin

Electron spin quantum # (ms=+1/2 or -1/2

Principle stating that no two electrons in an atom can have the same set of 4 quantum #'s

Pauli exclusion principle

Ground state electron configuration

Lowest energy arrangement of electrons

Electron configuration that lists subshells that contain electrons & designates their populations by what

Appropriate superscripts

Rule that states that for a partially filled subshell, the lowest energy arrangement will have the max # of unpaired electrons with the same spin state

Hund's rule

If all electrons in an atom are paired, the atom is not attracted by a magnet & is considered

Diamagnetic

If an atom has unpaired electrons, then the atom is attracted to a magnet & is considered

Paramagnetic

Principle that says you need to put electrons in the lowest energy orbitals before moving up

Aufbau principle

Periods arranged by

Increasing mass

Groups arranged by

Similar properties

Periodic table created by

Mendeleev & Meyer

Atomic number or mass more important?

Atomic number

Group 1A-7A, incompletely filled outer s or p shells

Representative elements

Group 8A, filled outer subshells (outer s and p shells filled)

Noble gases

Groups 1B and 3B-8B, incompletely filled outer d subshells

Transition metals

Neither representative nor transition metal elements, no special name for this group

Group 2B

Elements set off below the table, have incompletely filled f subshell

Lanthanides & Actinides

Ions & atoms with the same number of e- and the same ground state are called what

Isoelectronic

1/2 the distance between atomic nuclei

Atomic radius

Negatively charged e- are attracted by the + charged nucleus

Effective nuclear charge

Core electrons shield the outer shell electrons from what

+ nucleus

How to find Zeff

Z (#of protons) - S (#of core e-)

Minimum energy required to remove an e- from the ground state of a gaseous atom

Ionization energy

Greater e- affinity means a greater what

Tendency to gain an e-

Exam 4 Flashcards

(84 cards)