chap 3

Question 1

what is double slit experiment and by who?

Answer 1

thomas young-made ripples in water with pebbles and watched what occured on otherside of wall with slit btwn them and observed screen billow out in middle. did with two slits and saw two separate ripples appeared and hit each other at certain points, amplifying it and screen reflected that with ripples. now with particles being fired it was same at first but with double slit it didnt have ripple effect and only gas two arcs

Question 2

what was the electromagnetic spectrum and by who?

Answer 2

james clerk maxwell. full range of electromagnetic radiation, organized by frequency(backwards jank c) or wavelength(upsidedown y). left side gamma rays(10^-3), xrays(10^-1),ultraviolet(10),VISABLE(10^3), infared(10^5),microwave(10^7),radiowaves(10^11).

Question 3

formula for speed of light

Answer 3

frequency x wavelength= C(speed of light-3 x 10^8 m/s)

Question 4

relationship btwn wavelength, frequency and energy

Answer 4

short wavelength+high frequency= more energetic
long wavelength+low frequency=less energetic

Question 5

define quantum theoryand by who- planks version

Answer 5

max plank. electromagnetic radiation (radient energy) is quantized into “energy packets”(quanta). energy levels occur in STEPS.

Question 6

planks constant formula and energy formula

Answer 6

h= 6.626 x 10^-34 j•s (joule)
E=h•frequency(c-thing)

Question 7

define photoelectric effect and by who?

Answer 7

albert einstien. says light(em radiation) can also act like a particle and a wave (duality of light) put light through tube thing and and measured that ex violet light have shorter wavelength and higher frequency than red light

Question 8

define absorbtion/emission spectra and by who?

Answer 8

joseph von fraunhofer. put white light through sample through slit through prism and get dark blue to red spectrum has dark black lines through it. the patterns of light absorbed or emitted by a substance

Question 9

define hydrogen emmision spectrum and by who?

Answer 9

robert bunsen and gustav kirchhoff observed that light through bunsen burner has HYDROGEN EMMISSION SPECTRUM which has a few lines of color

Question 10

define hydrogen absorption spectrum and by who?

Answer 10

johann balmer and johannes rydberg put white light through H2 and through prism and got full color(blue to red) but with black lines in spots. (each element has unique lines)

Question 11

what was The bohr model and by who?

Answer 11

neils bohr. took balmer and rydbery measurements and planks quanta and found electrons are in circles around nucleus( n=1, n=2, n=3) excited electron absorbs EM radiation and makes the black lines. when electron gains energy it moves up a level +vice versa. explains H well but not others

Question 12

what is ground state?

Answer 12

lowest energy needed to keep electron stable (n=1)

Question 13

define ionization energy

Answer 13

electron gets enough energy to leave atom entirely and never come back

Question 14

define de broglie wavelengths and by who?

Answer 14

louis de broglie. asked why can electrons behave as waves? if n=3 the wavelengths line up but if n=2 1/2 the wavelengths don’t line up which is why electron cant go to the nucleus or in between phase

Question 15

define uncertainty principle and by who?

Answer 15

werner heisenberg. energy required to”see” an electron is much greater than the energy of an electron. can predict probability of where they exist but never fully precise

Question 16

wave mechanics by who? + symbol

Answer 16

Erwin schrödinger. mathematical approach that describes the wave-like behavior of electrons in atoms and molecules essentially treating electrons as both particles and waves, allowing for the prediction of their probable locations within an atom or molecule based on their wave functions. wave functions symbol looks like trident(psi) crazy math

Question 17

define orbital and formula and by who?

Answer 17

max born. is wave function(trident) squared. orbital is probability of where an electron can exist within a particular energy level.

Question 18

4 types of quantum numbers

Answer 18

principle quantum number, angular momentum quantum number, magnetic quantum number, spin quantum number

Question 19

define principle quantum number

Answer 19

corresponds to rows on periodic table. as you go higher in number energy increases and electron gets farther from nucleus. n=1,2,3,etc

Question 20

define angular momentum quantum number

Answer 20

l= integers from 0 to n-1
n=1 l=0. s-sublevel
n=2 l=0, 1. s+p sublevel
n=3 l=0, 1 2. s+p+d sublevel
n=4 l=0, 1,2,3 s+p+d+f sublevel

Question 21

define magnetic quantum number

Answer 21

specifies the orbital
ml=integers range from -1 to +1 and include zero
n=1 l=0 ml=0 so only 1 orbital at s sublevel
n=2 l=0,1 ml=0, -1 0 +1 so 3 orbitals at p sublevel
n=3 l=0,1,2 ml=0, -1 0 +1, -2 -1 0 +1 +2 so 5 degenerate orbitals at d sublevel
n=4 l=…3 ml=…-3 -2 -1 0 +1 +2 +3 so 7 degenerate orbitals at f sublevel

Question 22

define degenerate orbital

Answer 22

Electron orbitals having the same energy levels. non overlapping regions of probability

Question 23

define spin quantum number

Answer 23

every orbital contains up to two electrons. (ms)
“spin up” +1/2 “spin down” -1/2

Question 24

define pauli exclusion principle and by who?

Answer 24

wolfgang pauli. says no two electrons can share the same set of four quantum numbers(cannot exist in the same place at the same time) ex: He: 2 electrons
1(n),0(l),0(ml),+1/2(ms)
1(n),0(l),0(ml), -1/2(ms)

Question 25

define aufbau principle

Answer 25

order of filling orbitals by increasing energy levels

Question 26

define hunds rule

Answer 26

when we have degenerate orbitals each will be half filled and with same spin before any are full

Question 27

what do orbital diagrams do? +looks

Answer 27

shows electrons in orbitals (paired or unpaired) boxes with up and down arrows in them.

Question 28

what do electron configurations show? and looks

Answer 28

shows electrons in the sublevels not the orbitals.
2. 2. 6. 1. -(show #of e-)
ex:1s2s2p3s

Question 29

define valence electrons

Answer 29

electrons in the hughest principle energy level(shell) with electron involved in the formation of chemical bonds. can lose or gain electrons to have full outer shell. sharing e-=covalent bond

Question 30

define isoelectronic

Answer 30

when element has cation or anion to match up with nearest noble gas.
ex: Na+ , F-, O-2,Mg+2 =Ne

Question 31

define octet rule

Answer 31

s&p sublevels full=noble gas

Question 32

what are the periodic trends in atomic radius

Answer 32

decreases as you move from left to right across a period and increases as you move down a group

Question 33

characteristics of electromagnetic spectrum left to right

Answer 33

left: high energy(hurt) high frequency short wavelengths
right: low energy(harmless) low frequency long wavelengths

Question 34

formula for de broglie wavelength

Answer 34

wavelength= h/m(mass)v(speed
mv=momentum

Question 35

define electron affinity

Answer 35

how strongly electrons are attracted to an atom

Question 36

process of effective nuclear charge. (Zeff) and explains what

Answer 36

Zeff=(#of protons from nucleus)-(#of lower shell electrons sheildimg nucleus)
explains why atomic radius decreases left to right