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DAT-chemistry > chapter 24 > Flashcards

chapter 24 Flashcards

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1
Q

what is the atom

A

the basic building block of matter, representing the smallest unit of a chemical element

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2
Q

what are the subatomic particles

A

protons, neutrons and electrons

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3
Q

where are protons and neutrons located in an atom

A

nucleus

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4
Q

where are electrons located in an atom

A

outside the nucleus in the orbitals

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5
Q

what are compounds

A

atoms of more than one element

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6
Q

are atoms created or destroyed in a chemical reaction

A

No, they are separated combined or rearranged

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7
Q

mass of 1 proton

A

1 unified atomic mass unit (amu, u) =1 da

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8
Q

do protons and electrons weight he same

A

No protons are 1840x greater than electrons

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9
Q

what is the atomic # equal to

A

protons

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10
Q

mass of 1 neutron

A

1 da or 1 u

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11
Q

different isotopes have different number of what

A

neutrons

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12
Q

true or false the charge of protons and electrons are equal in magnitude but opposite in sign

A

true

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13
Q

valence electrons

A

electrons farthest in the electron shell

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14
Q

does attraction between the nucleus and the e increase or decrease in the valence electrons

A

decrease

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15
Q

what determines the reactivity of an atom

A

the valence electrons and their activity

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16
Q

what is an ion

A

the loss or gain of an e

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17
Q

what is the atomic mass number A equal to

A

total # of nucleons ( protons and neutrons-

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18
Q

what is the molecular weight

A

the weight in grams per 1 mole of a given element (g/mol)

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19
Q

what is avogadro’s number

A

6.02x1023 particles/mol

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20
Q

what is the standard atomic weight

A

a weighted average of all the isotopes of an element found naturally on earth

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21
Q

who is Ernest Rutherford

A

provided experimental evidence that an atom has a dense positively charged nucleus that accounts for only a small portion of the volume of atom

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22
Q

who is Max planck

A

developed the first quantum theory proposing that energy emitted as electromagnetic radiation from matter comes in discrete bundles called quanta

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23
Q

what is the equation of the energy value of a quantum

A

-eqn E=hf
h= Planks constant =6.626x10-34Js
f=frequency

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24
Q

what is the Bohr H model

A
  • consisted of a central proton around which an electron traveled in a circular orbit and that the centripetal force acting on the electron as it revolved around the nucleus was the electrical force between the positively charged proton and the negatively charged electron
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25
Q

what 2 ideas did Bohr combine to get the energy of the e

A

quantum theory of plancks and classical physics

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26
Q

what is the equation of the energy of electron

A
  • E=-RH/n2

o RH is constant called Rydberg energy

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27
Q

what causes the Electron energy to change

A

n=principal quantum number

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28
Q

is the energy of an electron is quantized

A

true

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29
Q

what are some characteristics of electrons using the Bohr model

A
  • The energy of the electron is related to its orbital radius: the smaller the radius the lower the energy state of the electron
  • The smallest orbit (radius) an electron can have corresponds to n=1 which is the ground state of the H electron
  • The ground state level the electron is in its lowest energy state
30
Q

at what temperature is majority of atoms in a sample are in the ground state

A

room temperature

31
Q

how can electrons be excited

A

by heat or other energy to yield the excited state of the atom

32
Q

what is released when an excited electron returns to ground state

A

energy in the form of photons

33
Q

what is the equation for the electromagnetic energy of photons

A

E=hc/wavelength
H= plancks constant
C=velocity of light in a vacuum =3.00x10^8 m/s
Wavelength of radiation

34
Q

what is the light spectrum

A

the spectrum quantized energy of light emitted does not produce a continuous spectrum but at is composed of light at specific frequencies
-Each line on the emission spectrum corresponds to a specific electronic transition

35
Q

what is the Atomic emission spectrum

A

ach element can have its electrons excited to different distinct energy levels so each element has its own atomic emission spectrum

36
Q

what are the Lyman series

A

n>1 n=1

spectrum region is ultraviolet

37
Q

what are the Balmer series

A

n>2 n=2

spectrum region visible and ultraviolet

38
Q

what are the Paschen series

A

n>3 n=3

spectrum region infrared

39
Q

what does this equation represent

–> E=hc/wavelength=-RH (1/ni2-1/nf2)

A

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

40
Q

When an electron is excited to a higher energy level it must absorb what

A

energy

41
Q

The most important difference between the Bohr model and modern quantum mechanical model

A

Bohr assumption that electrons follow a circular orbit at a fixed distance from the nucleus is no longer considered valid rather electrons are described as being in a state of rapid motion within regions of space around the nucleus called orbitals

42
Q

Heisenberg uncertainty principle

A

it is impossible to simultaneously determine with perfect accuracy the momentum ( defined as mass x velocity) and the position of an electron

43
Q

Modern atomic theory states that any electron in an atom can be completely described by 4 quantum numbers: what are they

A

n,l,ml, ms

  • N=size
  • L= shape
  • Ml= orientation
44
Q

Pauli exclusion principle

A

no 2 electrons in a given atom can possess the same set of 4 quantum numbers

45
Q

what is the energy state

A

the position and energy described by its quantum number

46
Q

what is Principle quantum number (n)

A
  • Positive integer value and represents the shell where an electron is
  • The max n that cann be used to describe the electron of an element at its ground state corresponds with that elements period ( row)
47
Q

what does n say about the energy level and radius of the electron

A

larger n= higher energy level and radius

48
Q

does the distance increase or decrease between shells as the distance from the nucleus increases

A

deceases

49
Q

what is azimuthal quantum number (angular momentum) (l)

A
  • the shape of the orbitals and refers to the subshells or sublevels that occur within each principle energy level
  • for an n the value of l can be integer in the range of 0 to n-1
50
Q

what are the 4 subshells corresponding to l=0,1,2,3

A

sharp (s), principle ( p), diffuse ( d), fundamental (f)

51
Q

the maximum number of electrons that can exist within a subshell is given by the equation?

A

4l+ 2

52
Q

what is the Magnetic quantum number (ml)

A
  • the orientation of the orbital in space
  • it specifies the particular orbital within a subshell where an electron is highly likely to be ofund at a given point in time
  • the possible values of ml are all the integers from l to –l including 0
53
Q

give the possible values of ml for subshell s

A

l=0 only has 1 possible value of ml=0 and will contain 1 orbital

54
Q

give the possible values of ml for subshell p

A

subshell l=1 has 3 possible values of ml -1,0, 1 and contains 3 orbitals

55
Q

give the possible values of ml for subshell d

A

has l=2 has 5 possible ml values and 5 orbitals

56
Q

give the possible values of ml for subshell f

A

l=3 has 7 possible values of ml and 7 orbitals

57
Q

what is spin quantum number (ms)

A
  • the spin of a particle is its intrinsic angular momentum and is a characteristic of a particle
  • spin orientations: +1/2 or -1/2
58
Q

according to what principle must 2 electrons in the same orbital must have opposite spins

A
  • the pauli exclusion principle
59
Q

parallel spins

A

electrons in different orbitals ( different ml values) with same ms value

60
Q

paired spins

A

electrons with opposite spins ( different ms values) in the same orbital ( same ml)

61
Q

what is the electron configuration

A

the first number denotes the principle energy level the letter designates the subshell and the superscript gives the number of e in that subshell

62
Q

aufbau principle

A

subshells are filled from lowest to highest energy and each subshell will fill completely before electrons begin to enter the next one

63
Q

what is the n+1 rule used for

A

to rank subshells by increasing energy

  • this rule states that the lower the sum of the first and second quantum numbers the lower the energy of the subshell
  • if 2 subshells possess the same n+l value the subshell with the lower n value has a lower energy and will fill first
64
Q

what is Hund’s rule

A

within a given subshell orbitals are filled such that there are a max number of half-filled orbitals with parallel spins

65
Q

paramagnetic material:

A

if the material has unpaired electrons a magnetic field will align the spins of these electrons and weakly attract the atom to the field

66
Q

diamagnetic material

A

material that have no paired electrons and are slightly replied by a magnetic field

67
Q

groups IA and IIA only the outermost valence electrons are

A

s electrons

68
Q

group IIA through VIIIA the outermost valence electrons are

A

s and p

69
Q

transition element the valence electrons are

A

outermost s subshell and in the d subshell of the next-to-outermost energy and f subshell of the energy shell 2 levels below the outer most shell

70
Q

true or false atoms with half-filled and fully filled subshells are not extremely stable

A

false

DAT-chemistry (4 decks)

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