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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

Protons have a mass of…

A

1 amu (atomic mass unit)

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2
Q

Z stands for

A

atomic number, the number of protons in an atom of an element

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3
Q

While all atoms of an element have the same atomic number, they do not necessarily have the same…

A

atomic mass due to isotopes!

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4
Q

A stands for

A

mass number, the sum of all protons and neutrons within an atom

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5
Q

Isotopes

A

atoms that have the same atomic number, but different mass numbers

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6
Q

Because subatomic masses are so small, electrostatic force of attraction between protons and electron is….

A

far greater than the gravitational force of attraction based on mass

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7
Q

Electrons close to the nucleus have..

A

lower energy levels and strongest interaction with nucleus

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8
Q

Electrons further away from the nucleus…

A

have higher energy levels and strongest interaction with the surrounding environment

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9
Q

Valence Electrons

A

electrons in the outer most shell of an atom, they determine the reactivity of an atom

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10
Q

Increase stability

A

having a full valence electron shell

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11
Q

Cation vs Anion

A

positively charged atom vs negatively charged atom

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12
Q

Atomic Mass/Mass Number

A

are synonymous! It varies from one isotope to another

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13
Q

Atomic Weight

A

Is constant for a given element; the weighted average of all isotope weights

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14
Q

Isotopes

A

when an element differs in the number of neutrons

but because protons and electrons are constant, they exhibit similar chemical principles

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15
Q

Half life corresponds with and helpd determine…

A

stability and helps determine proportions of isotopes

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16
Q

Avogadros Number

A
  1. 02*10^23 atoms/molecules /ions/things in 1 mole
    ex: 12 amu atomic weight of carbon means
  2. 02*10^23 atoms of carbon = 12 amu
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17
Q

Calculating Atomic Weight of an Unknown Element

A

(% Isotope 1)(atomic mass Isotope 1) + ….. = Atomic Weight

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18
Q

Ernest Rutherford

A

gave evidence that an atom has a dense, positively charged nucleus that is a small portion of atoms volume

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19
Q

Max Planck

A

developed first quantum thoery, energy emitted as electromagnetic radiation from matter comes from quanta

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20
Q

Planck Relation

A

E = hF

E = energy

h = plancks constant

f = frequency of radiation

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21
Q

Bohr Model Postulate

A

that centripetal force causing electrons to be in orbit is caused due to the electrostatic force between the positively charged protons and negatively charged electrons

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22
Q

Angular Momentums of an Electron Equation

A

L = nh/2pi

n = quantum number
h = plancks constant

angular momentum only changes with respect to the quantum number

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23
Q

Energy of an Electron

A

E = - Rh / n^2

Rh = rydberg unit of energy

Energy changes with respect to the quantum number like angular momentum

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24
Q

a value of 0 energy states that a proton and electron are…

A

not attracted at all, not close

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25
Q

Energy of an electron increases…

A

the farther from the nucleus it is (as quantum number increases)… think energy of an electron equation

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26
Q

Ground State

A

lowest electron energy

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27
Q

Excited State

A

highest electron energy as electron moves above to another shell further out

28
Q

How can electrons be excited?

A

via heat/energy forms

29
Q

Emission of photons

A

when excited form electrons drop back down to ground state, they emit energy in the form of photons

the photon emitted has a wavelength associated with it depending on the specific energy transmission

30
Q

Electromagnetic Energy of Photons

A

E = hc/ lambda

lamba = wavelength

h = Planck’s constant

31
Q

Atomic Emission Spectrum

A

each element can have its electrons excited to a different set of distinct energy levels giving them a unique atomic emission spectrum

32
Q

Lyman Series

A

group of hydrogen emission lines corresponding energy levels n greater than or equal to 2 to n = 1

33
Q

Balmer Series

A

group of hydrogen emission lines corresponding energy levels n greater than or equal to 3 to n = 2

34
Q

Paschen Series

A

group of hydrogen emission lines corresponding energy levels n greater than or equal to 4 to n = 3

35
Q

Lyman Series has larger energy transitions than Balmer series therefore it…

A

has shorter photon wavelengths

36
Q

Combining Planck’s and Bohr’s Theories states

A

The energy emitted photon corresponds to the difference in energy between the higher energy initial state and the lower energy final state

37
Q

Absorption spectrum

A

in addition to each element having a unique emission spectrum, they also each have a unique absorption spectrum

38
Q

Emission and Absorption Spectrum

A

uniques for each element, wavelength for each corresponds with one another because difference in energy levels is unchanged

39
Q

Quantum Mechanical Model

A

electrons move rapidly and are localized in regions of space around nucelus known as orbitals

40
Q

Heisenberg Uncertainty Principle

A

its impossible to determine perfectly the momentum and position of an electron

41
Q

Pauli Exclusion Principle

A

no two electrons in a given atom can possess the same set of 4 quantum numbers

42
Q

Principle quantum Number (n)

A

the larger the integer value of n (electron shell), the higher the energy level and radius of the electons shell

43
Q

Maximum number of Electrons Within a Shell

A

2n^2

44
Q

The difference in energy between two shells DECREASES as the distance from the nuclues ___

A

INCREASES

n=3 to n=4 is lower than n= 2 to n=3

45
Q

Azimuthal (Angular Momentum) Quantum Number (l)

A

refers to the shape and number of subshells within a principle energy level

l = all numbers less than n -1

ex: n=2 ; l = 1 or 0

this means there are 2 subshells (1 and 0) within the second principal energy level

46
Q 
l = 0
l = 1
l = 2
l = 3
A

s, p, d, f orbitals respectively

47
Q

Maximum Number of Electrons within a subshell =

A

4l + 2

48
Q

Magnetic Quantum Number (ml)

A

specifies the particular orbital within a subshell where an electron is most likely to be found at a given time

  • l , 0 , l
49
Q

s subshell orbital shape

p subshell orbital shape

A

s subshell have spherical orbitals

p subshell has 3 dumbell type orbitals

50
Q

As atomic number increases, so too does the number of….

A

electrons

51
Q

Spin Quantum Number (ms)

A

spin orientation +1/2 or -1/2

52
Q

Parallel Spins

A

Electrons in different orbitals with the same ms values

53
Q

Example: 2p^4

A

Indicates that 4 electrons in the second p subshell of second principal energy level is filled, also that all energy levels below 2p are filled

54
Q

Aufbau Principle

A

each subshell will fill completely before electrons enter the next one

55
Q

n + l rule

A

ranks subshells by increasing energy

the lower the sum of n+l,, the lower the energy of the subshell.

IF n+l are equal, then the subshell with the lower n has the lower energy and will fill first **pg 21

56
Q

***Subshells for cations

A

start with neutral element and then remove electrons from subshells with the highest n value

57
Q

Ex: electron configuration of Fe 3+

A

Neutral: [Ar] 4s^2 3d^6

Cation: [Ar]3d^5

58
Q

Hunds RUle

A

within a given subshell, orbitals are filled so maximum number of half-filled orbitals with parallel spins (each orbital has an electron before one is completely filled)

59
Q

Notable exceptions to Electron Config

A

Chromium and ELements in its group [Ar]4s13d4

Copper and elements in its group [Ar]4s13d10

60
Q

The presense of paired or unpaired electrons affects the….

A

chemical and magnetic properties of an atom or molecule

61
Q

Paramagnetic

A

unpaired electrons will orient their spins in alignment with a magnetic field and material will be attracted to the field

62
Q

Diamagnetic

A

materials with paired electrons will be slightly repelled y a magnetic field

63
Q

Valence ELectrons for Groups 13-18

A

highest s and p subshell electrons are the valence electrons

64
Q

Valence Electrons for Transition Elements

A

highest s and d subshell electrons

65
Q

All elements in period three (startng with sodium) and below may accept electrons into….

A

their d subshell and hold more than 8 electrons in the valence shell

Chemistry (9 decks)

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