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General Chemistry > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

what are the 2 classes of objects

A

matter and electromagnetic radiation

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2
Q

describe the characteristics of matter

A

-has both volume and mass
-has a defined position in space/time
-follows newton’s law

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3
Q

describe the characteristics of electromagnetic radiation

A
  • doesn’t have mass
  • delocalized and propagated through waves
    -follows maxwell’s equations
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4
Q

what’s the purpose of electromagnetic radiations

A

allows energy to travel through space

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5
Q

what are the 3 characteristics of electromagnetic radiation

A

1) wavelength (lambda): distance between two peaks/bottoms in waves
2) frenquency (mu): amount of waves/cycles per sec that pass at a given point
3) speed (C): speed of light

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6
Q

how are wavelenght and frenquency related

A

inversly proportional

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7
Q

define waves

A

continuous repeated change/oscillation through matter or a physical field

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8
Q

define light

A

a type of electromagnetic wave that contain oscillation through a magnetic field and that travels space

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9
Q

true or false
Energy can only be lost/gained through multiple integers

A

true

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10
Q

Whats Plank’s equation and its purpose

A

E=hv
gives us the electronic transiton of an electron

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11
Q

Why is energy considered to be quantized

A

system can only transfert energy whole quanta/packets

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12
Q

whats the photoelectric effect

A

when electrons are ejected fro a metal or other materials because light is shining on it.

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13
Q

Fill the blank
Light has both propertie of — and —

A

wave and matter

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14
Q

what is light’s duality

A

particle/wave duality

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15
Q

True or false
energy has matter and matter has energy

A

true

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16
Q

What two equation did De Broglie mix to fin the E of a photon

A

E=mc^2 and E=hv

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17
Q

what’s a continuous spectrum

A

a spectrum that emits all wavelengths of light (rainbow)

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18
Q

whats a line spectra

A

spectrum where only certain colors appear since only specific wavelengths are present
only certain energies are allowed for electrons.

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19
Q

what are the 4 main concepts of the atomic spectrum

A

1) electrons move from orbit to orbit, but its easier for them to go from an outter shell to inner one
2) the difference/distance between shells is the wavelength
3) energy is lost when electron transition between shells, that energy is carried out by photon which emit light
4) diff wavelength = diff colors

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20
Q

whats a ground state

A

lowest possible energy level (n=1), the closest to the nucleus and most stable since more attraction

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21
Q

define the energy level postulate

A

electrons can only be associated to specific energy levels

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22
Q

true of false
energy is absorbed when electrons move from outter shells to inner ones

A

false, the energy is omitted
for energy to be absorbed the electrons must move from inner to outer levels.

23
Q

what are the limitations of Bohr’s model

A

it only works for one elctron systems and doesn’t take in consideration the particle/wave duality of light

24
Q

what does the quantum mechanical model explain

A

it explain electrons according to the particle/wave duality

25
Q

what does shrodinger’s equation gives us

A

gives us the probability of finding an electron in a specific region of space.

26
Q

what does the principal quantum number (n) describe and what is its possible values

A

n= size and energy of shell, the smaller the value= smaller orbit and energy
values are positive integers above 0

27
Q

what does the angular momentum quantum number (l) describe and what is its possible values

A

l= distinguishes the different orbital shapes within an orbit
values range form 0 to n-1
values associated to differentes shapes

28
Q

what does the magnetic quantum number (ml) describe and what is its possible values

A

distinguishes the different orientation of orbitals
values: depends on values of l
(-l..,0,..l)

29
Q

what does the spin quantum number (ms) describe and what is its possible values

A

distinguishes the 2 differentes possible spins of an e-
values: -1/2 or 1/2

30
Q

define the pauli’s exclusion principle

A

no two electrons can have the same set of four quantum number and each orbital can hold up to 2 electrons and they must be of opposite spin

31
Q

whats a polyelectronic atom

A

atom with more than one electron, they usually follow the spdf order

32
Q

why do s orbital have lower energy than d or p orbitals

A

the closer an orbital is to the nucleus the less energy it has as the attraction between the nucleus and the electrons is stronger therefor it penetrates more

33
Q

define the Aufbau principle

A

since protons are added pne by one to build up the elements the electrons are added similarly in the orbital, one by one

34
Q

define Hund’s rule

A

the lowest energy configuration can only be obtained if we maximize the amount of unpaired electrons in orbitals

35
Q

where do we find valence electrons

A

in the outermost shell of the atom

36
Q

how does the atomic radius change and why

A

in a family the atomic radius increases as we go down since the number of orbit increases
in a period, as we go towards the right, the radius decreases since the number of proton increase with creates more attraction and therefor more condensed

37
Q

true or false
the atomic radius is the distance between two nuclei in a diatomic molecule

A

true

38
Q

whats the ionization energy and explain the trend across the periodic table

A

energy needed to remove the outermost electron to create a cation
as we go down a family it decreases and increases as we go towards noble gases

39
Q

true or false
the first ionization energy is the strongest

A

false its the weakest

40
Q

true of false
ionization energy and electron affinity involves atoms in every state

A

false on gaseous state

41
Q

define electron affinity

A

energy needed to add an electron to create an anion thats more stable

42
Q

What trends describe electron affinity

A

from left to right, energy becomes more exothermic
exothermic= electron added so energy released
endothermic = electron removed so energy added

43
Q

whats the difference between paramagnetic substances and diamagnetic substances

A

P= weakly attracted to a magnetic field since has unpaired electrons
D= not attracted to a magnetic field since has paired electron

44
Q

why are pair electrons not attracted to a magnetic field

A

since the paire electrons have opposite spins they cancel eachother and have no charge unlike an un paired electron

45
Q

whats the wavelength of microwaves and radar

A

microwaves= 10^-2 m
radar= 10^-1 m

46
Q

what the wavelength of far infrared

A

10^-4 m

47
Q

between what wavelengths is the visible light spectrum

A

between 350 and 800 nm

48
Q

whats the wavelength of near infrared

A

10^-5 m

49
Q

whats the wavelength of uv

A

10^-7 and 10^-8 m

50
Q

whats the wavelength of x rays

A

between 10^-9 and 10^-11 m

51
Q

whats the wavength of gamma rays

A

10^-12 m

52
Q

state all waves in order of decreasing wavelength

A

radar-microwaves-far infrared-near infrared- visible- near uv- far uv- x rays- gamma rays

53
Q

what are the two atoms with an exception in their last orbitals

A

Cr: 4s^1 3d^5
Cu: 4s^1 3d^10

54
Q

define ground state

A

lowest energy configuration possible
more stable

General Chemistry (9 decks)

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