Chapters 4-7 Midterm Review

Front 1

The distance between two successive peaks on adjacent waves is its _________.

Back 1

wavelength

Front 2

The frequency of electromagnetic radiation is measured in ________.

Back 2

hertz

Front 3

The product of the frequency and the wavelength of a wave equals the _______________.

Back 3

speed of the wave

Front 4

Max Planck proposed that a hot object radiated energy in small, specific amounts called _________.

Back 4

quanta

Front 5

The energy of a photon is related to its ________.

Back 5

frequency

Front 6

A quantum of electromagnetic energy is called a(n) _______

Back 6

photon

Front 7

The emission of electrons from metals that have absorbed photons is called the _________.

Back 7

photoelectric effect

Front 8

For an electron in an atom to change from the ground state to an excited state, energy must be ________.

Back 8

absorbed

Front 9

The change of an atom from an excited state to the ground state always requires the emission or release of ____________ __________.

Back 9

electromagnetic radiation

Front 10

A line spectrum is produced when an electron moves from one energy level to a ________ energy level.

Back 10

lower

Front 11

According to Bohr, where do electrons reside (where are they located)?

Back 11

electrons are located only in specific orbits (not between)

Front 12

If electrons in an atom have the lowest possible energies, the atom is in the ________.

Back 12

ground state

Front 13

The region outside the nucleus where an electron can most probably be found is the _________.

Back 13

electron cloud

Front 14

A three-dimensional region around a nucleus where an electron may be found is called a(n) __________.

Back 14

orbital

Front 15

A spherical electron cloud surrounding an atomic nucleus would best represent a _________ orbital.

Back 15

s

Front 16

The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called _______ orbitals.

Back 16

p

Front 17

How many orbitals are within the d sublevel?

Back 17

5

Front 18

The principle that states that an electron occupies the lowest available energy level is the ___________.

Back 18

Aufbau principle

Front 19

_______(#) electrons can occupy the s orbitals at each energy level. These electrons must have _________ spins.

Back 19

2, opposite

Front 20

List the atomic orbitals in the correct order they are filled. Start with 1s and go through 5s.

Back 20

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s

Front 21

The principle that requires that each of the orbitals at a particular energy level receive one electron before any of them can have two electrons is the ______.

Back 21

Hund's rule

Front 22

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to __________.

Back 22

Mendeleev

Front 23

What does the periodic law state?

Back 23

the physical and chemical properties of the elements are periodic functions of their atomic numbers

Front 24

Mendeleev arranged elements according to increasing __________.

Back 24

atomic mass

Front 25

The modern periodic table arranges elements according to increasing __________.

Back 25

atomic number

Front 26

To which group does iodine and bromine belong?

Back 26

halogens

Front 27

The elements in group 2 are also known as the ___________.

Back 27

alkaline earth metals

Front 28

The elements in group 1 are also known as the ___________.

Back 28

alkali metals

Front 29

The most reactive group of nonmetals is the __________.

Back 29

halogens

Front 30

The ________ are the radioactive elements with atomic numbers from 90 to 103.

Back 30

actinides

Front 31

The _________ are the elements with atomic numbers from 58 to 71.

Back 31

lanthanides

Front 32

Argon, krypton, and xenon are _________.

Back 32

noble gases

Front 33

__________ is the first member of the noble gas family whose highest energy level contains an octet of electrons.

Back 33

neon

Front 34

Elements in which the d sublevel is being filled have the properties of _______.

Back 34

metals

Front 35

Why is hydrogen placed separately from other elements in the periodic table?

Back 35

because of many of its unique properties

Front 36

To which block do the lanthanide and actinide elements belong?

Back 36

f block

Front 37

________ electrons are the electrons that are available to be lost, gained, or shared when atoms form compounds.

Back 37

valence

Front 38

For groups 13-18, the total number of electrons in the highest occupied level equals the group number minus _______.

Back 38

10

Front 39

How many valence electrons are in group 1 elements? Group 2?

Back 39

1, 2

Front 40

How many valence electrons are in group 16 elements? 17? 18?

Back 40

6, 7, 8

Front 41

__________ is the energy required to remove an electron from an atom.

Back 41

ionization energy

Front 42

A negative ion is known as a(n) _________.

Back 42

anion

Front 43

A positive ion is known as a(n) _________.

Back 43

cation

Front 44

A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called _________.

Back 44

electronegativity

Front 45

Which element has the greatest electronegativity?

Back 45

fluorine

Front 46

A _________ is a mutual attraction between the nuclei and valence electrons of different atoms that binds the atoms together.

Back 46

chemical bond

Front 47

The electrons involved in the formation of a chemical bond are called _________ electrons.

Back 47

valence

Front 48

The _________ are a group of elements that satisfy the octet rule without forming compounds.

Back 48

noble gases

Front 49

A neutral group of atoms held together by covalent bonds is a _______.

Back 49

molecule

Front 50

A __________ shows the types and numbers of atoms joined in a single molecule of a molecular compound.

Back 50

molecular formula

Front 51

As atoms bond with each other, they _________ (increase, decrease) their potential energy, thus creating _______(more, less) stable arrangements of matter.

Back 51

decrease, more

Front 52

A ________ molecule contains a region of positive charge and a region of negative charge.

Back 52

polar

Front 53

The ions in most ionic compounds are organized into a _________.

Back 53

crystal lattice

Front 54

Why are ionic compounds brittle?

Back 54

In a crystal lattice, even a slight shift of one row of ions relative to another causes a large buildup of repulsive forces causing the crystal to shatter

Front 55

Shifting the layers of an ionic crystal causes the crystal to _________.

Back 55

shatter

Front 56

__________ (ionic, molecular) compounds have higher melting and boiling points than ___________ (ionic, molecular) compounds.

Back 56

ionic, molecular

Front 57

A chemical bond formed by the attraction between positive ions and surrounding mobile electrons is a(n) __________ bond.

Back 57

metallic

Front 58

Compared with nonmetals, the number of valence electrons in metals is generally _________ (smaller, greater, the same).

Back 58

smaller

Front 59

In metallic bonds, the mobile electrons surrounding the positive ions are called a(n) _________.

Back 59

electron sea

Front 60

In metals, the valence electrons are _________ by all of the atoms.

Back 60

shared

Front 61

Malleability and ductility are characteristic of substances with _________ bonds.

Back 61

metallic

Front 62

If a material can be shaped or extended by physical pressure, such as hammering, which property does the material have?

Back 62

malleability

Front 63

Metals are ________ because the metallic bonding allows one plane of ions to slide past another.

Back 63

malleable

Front 64

To draw a Lewis structure, one must know the number of ___________ in each atom.

Back 64

valence electrons

Front 65

In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by _______ (#) electrons.

Back 65

8

Front 66

Multiple covalent bonds may occur in atoms that contain ________, _______, or __________.

Back 66

carbon, oxygen, and nitrogen

Front 67

Bonding in molecules or ions that cannot be correctly represented by a single Lewis structure is _________.

Back 67

resonance

Front 68

A _________ is placed between a molecule’s resonance structures to indicate resonance.

Back 68

double headed arrow

Front 69

The strong forces of attraction between the positive and negative regions of molecules are called _______ forces.

Back 69

dipole-dipole

Front 70

A chemical formula for a molecular compound represents the composition of a _________.

Back 70

molecule

Front 71

A chemical formula includes the ________ of the elements in the compound and the _________ that indicate the number of atoms or ions of each element that are combined in the compound.

Back 71

symbols, subscripts

Front 72

How many atoms of sulfur are present in a molecule of carbon tetrasulfide, CS4?

Back 72

4

Front 73

The _________ _______ of an element is the mass of one mole of the element.

Back 73

molar mass

Front 74

The molar mass of CaBr2 is the sum of the masses of _______(#) mol of Ca and _______(#) mol of Br.

Back 74

1, 2