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General Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is the charge of proton?

A

e = 1.6 x 10^-19 C

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2
Q

What is the mass of a proton?

A

one atomic mass unit (amu)

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3
Q

What is the atomic number?

A

(Z) number of protons, at top of element box

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4
Q

What is the mass number?

A

A - number of protons plus neutrons

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5
Q

What are isotopes?

A

atoms that share an atomic number but have different mass numbers are isotopes of the same element, differ in the number of neutrons

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6
Q

What is the mass of an electron compared to a proton?

A

about 1/2000 of that of the proton

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7
Q

What are valence electrons?

A

electrons in the outermost shell and can participate in bonds and most easily removed, “active”

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8
Q

What is a positively charged atom called?

A

cation

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9
Q

What is a negatively charged atom called?

A

anion

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10
Q

What is atomic mass?

A

also known as mass number, is the sum of protons and neutrons

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11
Q

What is atomic weight?

A

the weighted average of these different isotopes

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12
Q

What is Avogadro’s number?

A

Na = 6.02 x 10^23

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13
Q

What is Planck relation?

A 
E = hf
h = Plank's constant
f = frequency of radiation
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14
Q

What is Planck’s constant?

A

6.626x10-34 Js

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15
Q

What is the equation for angular momentum of electron orbiting a hydrogen nucleus?

A 
L = nh/2pi
n = principal quantum number
h = Planck's constant
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16
Q

What is the equation for the energy of the electron?

A 
E = -(Rh/n^2)
Rh = Rydberg unit of energy
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17
Q

What is Rydberg unit of energy?

A

2.18x10^18 J/electron

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18
Q

What is ground state?

A

atom is the state of lowest energy, in which all electrons are in the lowest possible orbits

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19
Q

What is excited state?

A

when at least one electron has moved to a subshell of higher than normal energy

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20
Q

Equation for electromagnetic energy of photons?

A 
E = hc/lambda
h = plancks constant
c= speed of light in vacuum
lambda = wavelength of radiation
21
Q

What is the value of c?

A

3.00 x 10^8 m/s - speed of light in a vacuum

22
Q

What is the line spectrum?

A

each line on the emission spectrum corresponds to a specific electron transition

23
Q

What is the atomic emission spectrum?

A

energy emitted from excited to ground state is exactly equal to the energy difference between the two levels - unique for every element

24
Q

What is Lyman series?

A

group of hydrogen emission lines corresponding to transitions from energy levels n>= 2 to n= 1

25
Q

What is the Balmer series?

A

group of hydrogen emission lines corresponding to transitions from energy levels n>= 3 to n=2

26
Q

What is the Paschen series?

A

group of hydrogen emission lines corresponding to transitions from energy levels n>= 4 to n=3

27
Q

What is an absorption spectrum?

A

exciting the electrons of a specific element results in energy absorption at specific wavelengths

28
Q

Difference between Bohr’s model of the atom and the modern quantum mechanical model?

A

Bohr believed that electrons followed a clearly defined circular pathway or orbit at a fixed distance while the modern theory knows that electrons move rapidly and are within regions of space around the nucleus

29
Q

What is an orbital?

A

regions of space around the nucleus

30
Q

What is the Heisenberg uncertainty Principle?

A

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

31
Q

What is the Pauli exclusion principle?

A

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

32
Q

What are the quantum numbers?

A

Principal (n)
Azimuthal/Angular momentum (l)
Magnetic Quantum Number (ml)
Spin Quantum Number (ms)

33
Q

What is the principal quantum number?

A

n designates the principal electron shell - or the number of shells around the nucleus?
max number of e- within a shell = 2n^2

34
Q

What is the angular momentum quantum number?

A

l - shape and number of subshells
l = n- 1
Max number of e- within a subshell = 4l+7

35
Q

What is the magnetic quantum number?

A

ml
a particular orbital within a subshell where an e- is most likely to be found at a given moment in time
-orbitals hold max 2e-
ml = -1 to +1

36
Q

What is the spin quantum number?

A

ms

only two spin designations - +1/2 or -1/2

37
Q

Electron configuration

A

the pattern by which subshells are filled, as well as the number of electrons within each principal energy level and subshell

38
Q

Spectroscopic notation

A

first number - denotes principle energy level
letter - designates the subshell
superscript - gives # of e- in the subshell

39
Q

What is Aufbau principle?

A

electrons fill from lower-to-higher energy subshells and each subshell is completely filled before electrons begin entering the next one

40
Q

What is the n+l rule?

A

the lower of the sum of the values of the first and second quantum numbers, n+l, the lower the energy of the subshell

41
Q

What does s equal?

A

l = 0

42
Q

What does d equal?

A

l =2

43
Q

What does p equal?

A

l = 1

44
Q

What does f equal?

A

l = 3

45
Q

What is Hund’s rule?

A

in subshells that contain more than one orbital will fill such that there is a maximum number of half-filled orbitals with parallel spins. half-filled and fully filled orbitals have lower energies and are more stable

46
Q

What are two elements with exceptions to electron configuration?

A

chromium and copper

47
Q

Paramagnetic

A

Atom or substance containing unpaired electrons and is consequently attracted by a magnet.

48
Q

Diamagnetic

A

materials consisting of atoms that have only paired electrons will be slightly repelled

General Chemistry (8 decks)

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