Chemistry Ch.4&5

Front 1

Describe the electromagnetic spectrum

Back 1

Radio waves, Microwaves, Infrared, Visible light, Ultraviolet, Xrays, Gamma rays

Front 2

What has the shortest wavelength and highest energy? What has the longest wavelength and lowest energy?

Back 2

1. Gamma rays 2. Radio waves

Front 3

When an electron switches energy levels to a higher orbital, is it releasing or absorbing energy?

Back 3

absorbing

Front 4

When an electron falls down to a lower state, does it release or absorb energy?

Back 4

releases

Front 5

produced by an atom in an excited energy state

Back 5

emission line

Front 6

a form of energy that exhibits wavelike behavior as it travels through space

Back 6

electromagnetic radiation

Front 7

all the forms of electromagnetic radiation

Back 7

electromagnetic spectrum

Front 8

the distance between corresponding points on adjacent waves

Back 8

wavelength

Front 9

the number of waves that pass a given point in a specific time, usually one second

Back 9

frequency

Front 10

refers to the emission of electrons from a mater when light shines on the metal

Back 10

photoelectric effect

Front 11

the minimum quantity of energy that can be lost or gained by an atom

Back 11

quantum

Front 12

the lowest energy state of an atom is its

Back 12

ground state

Front 13

a state in which an atom has a higher potential energy than it has in its ground state is an

Back 13

exited state

Front 14

When a narrow beam of emitted light was shined through a prism, it was separated into four specific colors of the visible spectrum. The four bands of light were part of what is known as hydrogen's ______.

Back 14

emission-line spectrum

Front 15

a continuous range of frequencies of electromagnetic radiation

Back 15

continuous spectrum

Front 16

Compare and contrast the continuous spectrum and the emission-line spectrum.

Back 16

The continuous spectrum is a continuous bright region with all the wavelengths of the selected region present.

An emission spectrum has only bright lines in a wide dark region corresponding to the photons absorbed and emitted by the electrons.

Front 17

occurs when matter emits electrons upon exposure to electromagnetic radiation, such as photons of light

Back 17

photoelectric effect

Front 18

Describe the Bohr model of the atom and the quantum mechanical model of the atom- compareand contrast the two models.

Back 18

In one model, the diffraction pattern produced by a beam of electrons passed through a substance. In the second model, diffraction pattern for a beam of visible light passed through a tiny aperture.

First model - light more spread out and blurred together

Second model - light in rings more separated by dark color

Front 19

states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle

Back 19

Heisenberg uncertainty principle

Front 20

describes mathematically the wave properties of electrons and other very small particles

Back 20

quantum theory

Front 21

a three-dimensional region around the nucleus that indicates the probable location of an electron

Back 21

orbital

Front 22

specify the properties of atomic orbitals and the properties of electrons in orbitals

Back 22

quantum numbers

Front 23

indicates the main energy level occupied by the electron, symbolized by n

Back 23

principal quantum number

Front 24

indicates the shape of the orbital, symbolized by l

Back 24

angular momentum quantum number

Front 25

indicates the orientation of an orbital around the nucleus, symbolized by m

Back 25

magnetic quantum number

Front 26

has only two values (+1/2,-1/2) which indicate the two fundamental spin states of an electron in an orbital

Back 26

spin quantum number

Front 27

the arrangement of electrons in an atom

Back 27

electron configeration

Front 28

an electron occupies the lowest-energy orbital that can receive it

Back 28

Aufbau principle

Front 29

no two electrons in the same atom can have the same set of h=four quantum numbers

Back 29

Pauli exclusion principle

Front 30

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin state

Back 30

Hund's rule

Front 31

the Group 18 elements (helium, neon, argon, krypton, xenon, and radon) are called

Back 31

the noble gases

Front 32

refers to an outer main energy level occupied, in most cases, by 8 electrons

Back 32

noble-gas configuration

Front 33

Mendeleev's principle of chemical periodicity correctly stated here; the physical and chemical properties of the elements are periodic functions of their atomic numbers

Back 33

periodic law

Front 34

an arrangement of the elements in order of their atomic numbers so the elements with similar properties fall in the same column or group

Back 34

periodic table

Front 35

14 elements with atomic numbers from 58-71; similar in chemical and physical properties

Back 35

lanthanides

Front 36

14 elements with atomic numbers from 90-103; set off below the main portion of the periodic table to save space

Back 36

actinides

Front 37

elements of group 1 on the periodic table (lithium, sodium, potassium, rubidium, cesium, and francium)

Back 37

alkali metals

Front 38

elements of group 2 on the periodic table (beryllium, magnesium, calcium, strontium, barium, and radium)

Back 38

alkaline-earth metals

Front 39

the d-block elements are metals with typical metallic properties

Back 39

transition metals

Front 40

the p-block elements together with the s-block elements

Back 40

main-group elements

Front 41

the elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine)

Back 41

halogens

Front 42

may be defined as one-half the distance between the nuclei of identical atoms that are bonded together (the trend to smaller atoms across a period charge of the nucleus)

Back 42

atomic radius

Front 43

an atomic group of banded atoms that has a positive or negative charge

Back 43

ion

Front 44

any process that results in the formation of an ion

Back 44

ionization

Front 45

the energy required to remove one electron from a neutral atom of any element

Back 45

ionization energy

Front 46

the energy change that occurs when an electron is acquired by a neutral atom is called the atom's

Back 46

electron affinity

Front 47

a positive ion is known as a

Back 47

cation

Front 48

a negative ion is known as an

Back 48

anion

Front 49

the electrons available to be lost, gained, or shared in the formation of chemical compounds are referred to as

Back 49

valence electrons

Front 50

a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound (tends to increase across each period)

Back 50

electronegativity

Front 51

How many valence electrons are in Groups number 1,2,13-18?

Back 51

1-1

2-2

3-3

14-4

15-5

16-6

17-7

18-8