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college chem > chaper 2 > Flashcards

chaper 2 Flashcards

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1
Q

light

A

light is a kind of electromagnetic radiation that can be described as a wave composed of oscillations mutually perpendicular electronic and magnetic fields propagating through space

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2
Q

light moves through any medium at a constant speed

A

c

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3
Q

amplitude

A

a (how high the wave crest is)

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4
Q

wavelength (lambda)

A

distance from peak to peak

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5
Q

frequency

A

the number of wavelengths in one second

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6
Q

c=

A

(wavelength)*(frequency)

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7
Q

light can be described(particle)

A

as traveling packets of light called photons

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8
Q

light can be described(wave)

A

energy can be transfered int o something

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9
Q

wave particle duality

A

energy can be transfered into a substance and it will emit light

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10
Q

emition spectrum

A

the collective wavelengths of visable lightemitted by a given element

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11
Q

explain the dual slit experiment

A

hs

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12
Q

heizenberg uncertanty principle

A

it is impossible to know both the position and velocity of an electron at any given time.

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13
Q

rainbolt uncertanty principle

A

i can actually be funny and i can think i’m being funny but never both at the same time.

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14
Q

orbital

A

the region of space where you will find a specific electron 90% of the time

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15
Q

s orbitals I=0

A

appears as a sphere

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16
Q

p orbitals I=1

A

looks like a peanut. symmetric about an axis

the axis they are on is the subscript after P

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17
Q

D orbital I=2

A

normally looks like a 4 leaf clover across 2 axis’
-the bubbles are in the quadrants of the 2 axi
-when they are on the axi the subscript becomes –squared and subtracted
also can be a peanut with a hoola hoop on the z^2 axis

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18
Q

f orbital I=3 passifiers

A

double passifires form on a respective axis

F z^3-3/5z(r^2)

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19
Q

f orbitals clover base

A

there is one that has a ballon in each 3d quadrant this is the xyz one

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20
Q

f orbiutal clover special

A

8 clovers lined wwith teh axis perpendicular to central

f(chentral axis z)(x^2-Z^2)

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21
Q

photon

A

a packet of light

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22
Q

how is the energy of a photon related to its wavelength

A

E=(h*c)/(wavelength)

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23
Q

how is the energy of a photon related to its frequency

A

E = h*(frequency)

24
Q

angular momentum quantum number (I)

A

this number determines spdf

25
Q

What are the possible values of the angular momentum quantum number l?

A

all the non-negative integers: 0,1,2,…, n-1, where n is a principal quantum number

26
Q

What does the angular momentum quantum number determine?

A

the shape of the orbital

27
Q

Why are atoms usually portrayed as spheres when most orbitals are not spherically shaped?

A

The shape of an atom is obtained by superimposing all of its orbitals.

28
Q

calculating frequency using wavelength

A

use the Eq v=c/(wavelength)

29
Q

Describe the interference pattern that results from the diffraction of electrons passing through two closely spaced slits.

A

The diffraction between electrons as they travel though 2 closely placed slits is an example of wave particle duality. When the electrons are not being monitored with a laser and are being measured for velocity, then they exhibit a wave like nature. However when the electrons are being measured for their position then they exhibit the traits of a particle. This led to the Heisenberg uncertainty principle which states that we can either know the position or the velocity of an electron at any given time, but we can never know them both at the same time. Electrons interfere with themselves when they are not being monitored for position and act with wave like interference when they are being monitored for velocity.

30
Q

Compare the characteristics of 4d orbitals and 3d orbitals and complete the following sentences.

A

4d orbitals would have more nodes and be larger in size than 3d orbitals.

31
Q

principle Quantum number

A

an integer that determines the size and energy of an orbital

32
Q

What are the possible values of the principal quantum number n?

A

all the positive integers: 1,2,3, etc.

33
Q

magnetic quantum number (Ml)

A

this is an interger that determines the orientation of the orbital. it ranges as the interger values in between -I and I

34
Q

spin quantum number

A

the spin Quantum number determines the electron spin and if it is spin up or spin down

35
Q

List all the orbitals in n=1. Specify the three quantum numbers for each orbital.

A

n=1,I=0,ml=0

36
Q

List all the orbitals in n=2. Specify the three quantum numbers for each orbital.

A

n=2; l=0; ml=0

n=2; l=1; ml=-1, 0, 1

37
Q

List all the orbitals in n=3. Specify the three quantum numbers for each orbital.

A

n=3, l=0; ml=0
n=3; l=1; ml=-1,0,1
n=3; l=2; ml=-2,-1,0,1,2

38
Q

List all the orbitals in n=4. Specify the three quantum numbers for each orbital.

A

n=4; l=0; ml=0
n=4; l=1; ml=-1,0,1
n=4; l=2; ml=-2,-1,0,1,2
n=4; l=3; ml=-3,-2,-1,0,1,2,3

39
Q

Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital?

A

2s

40
Q

when electrons move to a higner electron what did it absorb or give up energy

A

it absorbed energy

41
Q

when an electron regresses to a lower electron level did it absorb or give off energy

A

it released energy

42
Q

what transitions result in ultraviolate rays

A

any level down to n=1

43
Q

what transitions result in visable wavelengths

A

any level<=6 to 2

44
Q

what transitions result in infared wavelengths

A

levels 5 and 4 to level 3

45
Q

what happens when an electron in shell 1 absorbs alot of energy

A

When an atom absorbs energy, the electron usually quickly relaxes to a lower level, emitting light. The color of the emission is determined by the energy difference between energy levels.

46
Q

how many electrons fit in an s orbital

A

2

47
Q

how many electrons fit in an p orbital

A

6 (3 boxes)

48
Q

how many electrons fit in an d orbital

A

10 (5boxes)

49
Q

how many electrons fit in an f orbital

A

14 (7boxes)

50
Q

diagram for filling up orbitals

A

rememeber it dammit draw it now. rate it on that

51
Q

how to write the electron configuration of an element

A

find the number of protons and then write it as 1s^22s^22p^6 etc

52
Q

how do do electron configuration with noble gasses

A

put the noble gas in brackets then start form there

53
Q

how to determine wether an element will become a cation or an anion

A

see if they are closer to a noble gas on the right or left

54
Q

orbital diagram

A

the box one

55
Q

electron configuration

A

the number one

56
Q

how to tell the shell based on the periodic table

A

look at the rows

57
Q

how to tell the number of valence electrons based on the periodic table

A

it has to do with the row that the elements are in. ex the 13th collum has 3

college chem (15 decks)

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