Unit 2 #2 Flashcards Preview

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Flashcards in Unit 2 #2 Deck (50):
1

gamma

10 to the -12

2

radio waves

100 meters

2

frequency

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

3

x ryas

10 to the -10

3

waves

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

4

microwaves

10 to the -2

4

speed

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

5

infared

10 to the -4

6

visbile light

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

7

bohr model

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

8

see red light

from 1 to 3

9

see green light

from 4 then 2

10

see blue light

from 5 to 2

11

energy =....

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

12

z

atomic number

13

ultraviolent

10 to the -8

13

speed of light

700 miles per hour

13

electro mangetic radiation

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

13

speed of light

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

16

Rh

riburg constant
always 2.178 times 10 to the -18 Joules

18

emission of light by excited hydrogen atoms

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

19

continous spectrum

white light pass through prism, continas all the wavelengths

20

line spectrum

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

21

Bohr

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

22

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

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)

23

ground state

lowest possible energy state

24

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

indicates that the atom has lost energy

25

aufbau principle

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

26

Hund's rule

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

27

valence electrons

electrons in the outermost principal quantum level of an atom

28

core electrons

inner electrons

29

orbital diagram

ARROWS

30

transition metals

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

31

important points of the periodic table

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

32

inoization energy

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

33

first inoization energy

energy required to remove the highest energy of an electron

34

second inoization energy

energy required to removed the second electron

35

when you go to the right....

the first ionization energy increasesoo

36

when you go down a group.....

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

37

electron affinity

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)

38

when go left to right (electron affinity)

electron affinity began negative

39

when you go down by group (electron affinity0

electron affinity become positive( (less energy released)

40

atomic radius

atom size cannot specify exactly

41

values for atomic radii

obtained distance between atoms in chemical compounds

42

when left to right (raddi)

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

43

when go down a group (radii)

atomic radii increaes

44

metals

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

45

nometals

right side, gain electrons form anions (negative)

46

metalloids

have metal and nonmetal properties

47

alkali metals

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