Unit 2 #2

Question 1

gamma

Answer 1

10 to the -12

Question 2

radio waves

Answer 2

100 meters

Question 2

frequency

Answer 2

write with letter n, number of waves per second, that pass a given point in space

Question 3

x ryas

Answer 3

10 to the -10

Question 3

waves

Answer 3

Greek letter that is upside down, distance between two consecutive peaks (1 full cycle), light is a wave

Question 4

microwaves

Answer 4

10 to the -2

Question 4

speed

Answer 4

C, speed of the waves, all electro magnetic waves travel at the speed of light

Question 5

infared

Answer 5

10 to the -4

Question 6

visbile light

Answer 6

in between
4 times 10 to the -7 and ….
7 times 10 to the -7

Question 7

bohr model

Answer 7

1.said there is a nucleus and different levels, 2. electrons confined to these levels, 3. when one passes energy through the tube, it takes it to another level and then drops down, 4. electron moves from high level to low levels, in doing so it releases an energy (photon) of light

Question 8

see red light

Answer 8

from 1 to 3

Question 9

see green light

Answer 9

from 4 then 2

Question 10

see blue light

Answer 10

from 5 to 2

Question 11

energy =….

Answer 11

photon’s constant times frequency, can use this to make calculations

Question 12

z

Answer 12

atomic number

Question 13

ultraviolent

Answer 13

10 to the -8

Question 13

speed of light

Answer 13

700 miles per hour

Question 13

electro mangetic radiation

Answer 13

includes light, x rays, micro waves, radio waves, all classified based on wave length

Question 13

speed of light

Answer 13

wave length (meters) times frequency (1/second)

Question 16

Rh

Answer 16

riburg constant

always 2.178 times 10 to the -18 Joules

Question 18

emission of light by excited hydrogen atoms

Answer 18

1. sample of hydrogen recieve high energy of spark
2. hydrogen molecule absorb energy and bonds are broken
3. they then get exicted
4. they release extra energy by wavelengths to produce emission spectrum of hydrogen atoms

Question 19

continous spectrum

Answer 19

white light pass through prism, continas all the wavelengths

Question 20

line spectrum

Answer 20

visible region passed through prism only see a few, indicates that only certain energies are alowed for the electron in the hydrogen atom

Question 21

Bohr

Answer 21

developed quantum model for the HYDROGEN atom, believed the electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits, gave hydrogen atom energy levels consistent with the hydrogen emission spectrum

Question 22

the negative in the equation (energy levels available to the electron in the hydrogen atom)

Answer 22

energy of the electron is lower than it would be if the electron were at an infinite distance from the nucleus (interation and energy = zero)

Question 23

ground state

Answer 23

lowest possible energy state

Question 24

the negative in the equation (the change in energy when the electron falls from one level to another

Answer 24

indicates that the atom has lost energy

Question 25

aufbau principle

Answer 25

as protons are added on by one to the nucleus to build up the elements, electrons are simply added to these hydrogenlike orbitals

Question 26

Hund’s rule

Answer 26

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by Pauli principle in a paritcular set of degenerate orbitals

Question 27

valence electrons

Answer 27

electrons in the outermost principal quantum level of an atom

Question 28

core electrons

Answer 28

inner electrons

Question 29

orbital diagram

Answer 29

ARROWS

Question 30

transition metals

Answer 30

configurations are obtained by adding electrons to the five 3d orbitals

Question 31

important points of the periodic table

Answer 31

1. (n + 1)s orbitals always fill before nd orbitals 2. lanthaninde series or lanthanides (filling of the seven 4f orbitals) 3.actinide series (filling seven 5f orbitals) 4. group label tells the total number of valence electrons for that gro

Question 32

inoization energy

Answer 32

required to remove an electron from a gaseous atom or ion, highest energy electron (one bound least tightly) is removed first

Question 33

first inoization energy

Answer 33

energy required to remove the highest energy of an electron

Question 34

second inoization energy

Answer 34

energy required to removed the second electron

Question 35

when you go to the right….

Answer 35

the first ionization energy increasesoo

Question 36

when you go down a group…..

Answer 36

first innozation decreases (electrons being removed are farther away from the nucleus)

Question 37

electron affinity

Answer 37

energy charge associated with addition of an electron to a gaseous atom (if addition of energy resutls in lower energy, the electron affinity will carry a negative sign)

Question 38

when go left to right (electron affinity)

Answer 38

electron affinity began negative

Question 39

when you go down by group (electron affinity0

Answer 39

electron affinity become positive( (less energy released)

Question 40

atomic radius

Answer 40

atom size cannot specify exactly

Question 41

values for atomic radii

Answer 41

obtained distance between atoms in chemical compounds

Question 42

when left to right (raddi)

Answer 42

atomic radii decreases, valence electrons become closer, decreasing in size

Question 43

when go down a group (radii)

Answer 43

atomic radii increaes

Question 44

metals

Answer 44

left side, cations (give up electrons, become postivie)

Question 45

nometals

Answer 45

right side, gain electrons form anions (negative)

Question 46

metalloids

Answer 46

have metal and nonmetal properties

Question 47

alkali metals

Answer 47

group 1A, going down (first inozation energy decreases, radii increaes), very reactive, low inoziation energy