Chapter 1 Atomic Structure Flashcards

1
Q

E(energy of photon)

A

hc/wavelength, RH[1/n2-1/n2(final)]

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2
Q

h

A

Planck’s constant=6.626x10^-34j*s

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3
Q

c

A

speed of light in vacuum 3x10^8 m/s

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4
Q

Mass number(A)

A

The sum of protons and neutrons

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5
Q

Atomic Weight

A

The weighted average of all isotopes, and is the number reported on the periodic table.

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6
Q

Rydberg unit of energy

A

(R(H)=-2.18x10^-18 J/electron

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7
Q

Heisenberg uncertainty principle

A

We cannot know both the position and speed of a particle such as a photon, or electron with perfect accuracy

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8
Q

Pauli exclusion principle

A

No two electrons in a given atom can possess the same set of four quantum numbers

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9
Q

Principal Quantum Numbers

A

(n)= used in bohrs model, the energy level of the electron orbitals. Any positive integer. The difference in energy between 2 shells=(1/n(i)^2)- (1/n(f)^2)

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10
Q

Second Quantum number

A

(l) (azimuthal or angular momentum quantum number). Possible values of l=(n-1)=tells you the number of subshells. l=0(s), l=1(p), l=2(d), l=3(f)
maximum number of electrons in subshell =4(l)+2

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11
Q

Third Quantum number

A

m(l) is magnetic quantum number specifying the orbital in a subshell.
s=0, p=-1,0,1, d=-2,-1,0,1,2, f=3

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12
Q

Fourth Quantum number

A

m(s) spin quantum #(+1/2)(-1/2)

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13
Q

Aufbau Principle

A

(building up principle)
each subshell will fill completely before electrons begin to enter the next one.

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14
Q

n=l rule

A

lower energy subshells will fill first

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15
Q

Hund’s Rule

A

Within a given subshell, orbitals are filled such that there are a maximum number of half-filled orbitals with parallel spins.

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16
Q

Avogadro’s number

A

6.02x10^23