Atomic Structure Flashcards

1
Q

e

A

1.6 x 10^-19 C

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2
Q

Atomic number

A

at the top
Equal to number of protons found in an element

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3
Q

Mass number

A

Lower number
Sum of protons and neutrons

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4
Q

Isotopes

A

Atoms that share an atomic number but have different mass numbers/numbers of neutrons

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5
Q

High vs lower electron shells

A

further higher energy vs closer lower energy

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6
Q

Sharing or transferring valence electrons

A

Can increase elements stability by filling their highest energy level

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7
Q

Atomic weight

A

Weighted average of different isotopes

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8
Q

Avogadro’s number

A

6.022 x 10^23

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9
Q

Planck’s relations (energy of a quanta)

A

E = hf
h= 6.626 x 10^-34 Js

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10
Q

Bohr’s law of energy of the electron

A

E = -R(H)/(n^2)
R(H) Rydberg 2.18 x 10^-18 J/electron

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11
Q

Ground state

A

n = 1

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12
Q

Excited state

A

e- promoted to a higher orbit/moved to a sub shell of higher than normal energy

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13
Q

Formulas to determine the electromagnetic energy emitted in the form of a photon when electron returns to ground state

A

E = hc/wavelength
c = 3 x 10^8 m/s
E = hf
E = R(H) x [ 1/(ni^2) - 1/(nf^2) ]

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14
Q

emission spectrum

A

Love nf = 1 (122, 103, 97, 95, 94)
Big nf = 2 (660, 490, 430, 410)
Penis nf = 3 (1900, 1300, 1100)

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15
Q

1 R(H) is equal to…

A

13.6 eV/electron

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16
Q

Heisenberg Uncertainty Principle

A

It is impossible to simultaneously determine with perfect accuracy, the momentum and the position of an electron

17
Q

Pauli exclusion principle

A

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

18
Q

Energy state

A

The position and energy of an electron described by its quantum numbers

19
Q

n

A

Principal quantum number
Can take on any positive integer value
The larger the n the higher the energy level and radius of the electron’s shell

20
Q

maximum number of electrons within a shell

21
Q

Difference in energy between two shells

A

[1/(ni^2)] - [1/(nf^2)]

22
Q

l

A

azimuthal quantum number
Describes shape and # of subshells within a given principal energy level
range: 0 to (n-1)
l=0 is called s (circle)
l=1 is called p (dumbbell)
l=2 is called d
l=3 is called f

23
Q

maximum number of electrons within a subshell

24
Q

ml

A

Magnetic quantum number
Specifies the orbital within a subshell where an electron is most likely to be found at a given moment in time
range: -l ~ +l

25
How can p subshells be oriented?
x, y, and z
26
number of orbitals in a subshell
2l + 1
27
ms
spin quantum number +1/2 or -1/2 - when two electrons are in the same orbital, they must have opposite spins (paired) - electrons in different orbitals with the same ms values are said to have parallel spins
28
Aufbau principle
each subshell will begin filling up before beginning to enter the next one n+l rule: the lower the sum of n and l the lower the energy of the subshells, if two subshells posses the same sum then the one with the lower n has a lower energy and will fill w electrons first
29
Hund’s rule
Take up solo spots in the orbitals within a subshell until they NEED to double up
30
What are the exceptions to Hund’s Rule?
chromium’s group and copper’s group you move an s electron to the d subshell to make it half full or full
31
Paramagnetism
materials composed of atoms with unpaired electrons will orient their spins in alignment with a magnetic field
32
Diamagnetism
Materials consisting of atoms that have only paired electrons will be slightly repelled by a magnetic field
33
Cation electron loss rule
electrons lost come from highest energy shell (n+l rule)