TEAS 7 - Science (Atomic Structure)

Question 1

An ____ is the smallest unit of matter.

Answer 1

atom

Question 2

The ___ is the center of the atom, which is made up of protons and neutrons

Answer 2

nucleus

Question 2

What are the two numbers that make up the atomic mass?

Answer 2

protons and neutrons

Question 2

A ___is a neutrally charged subatomic particle; it is located in the nucleus at the center of the atom

Answer 2

neutron

Question 2

The atomic number of elements on the Periodic Table of Elements is the element’s ___ ___.

Answer 2

atomic number

Question 2

An ___ is a negatively charged subatomic particle that moves around the outside of the nucleus of an atom along circular paths called orbitals.

Answer 2

electron

Question 3

A ___ is a positively charged subatomic particle; the number of protons gives an atom its identity; it is located in the nucleus at the center of an atom

Answer 3

proton

Question 4

What is the smallest unit of matter?

Answer 4

atoms

Question 4

___ are imaginary paths surrounding the nucleus of an atom along which electrons travel; each orbital has a different level of energy and can hold a certain number of electrons

Answer 4

Orbitals

Question 4

What is the charge of a proton? Neutron? Electron?

Answer 4

Proton: (+)

Neutron: none

Electron: (-)

Question 4

The ___ ___ is the area around the nucleus of an atom that contains electrons traveling around the nucleus.

Answer 4

electron cloud

Question 5

The physical structure of an atom is fairly simple: a ___ at the center (which is composed of ___ and ___) and ___ orbiting the nucleus in an area often called the “electron cloud.”

Answer 5

nucleus

protons

neutrons

electrons

Question 6

The ___ is located at the center of an atom.

Answer 6

nucleus

Question 7

What is the nucleus made of?

Answer 7

protons and neutrons

Question 8

___ have a positive charge.
___ have a neutral charge.
___ have a negative electrical charge.

Answer 8

Protons
Neutrons
Electrons

Question 9

What obits the nucleus in rings?

Answer 9

electrons

Question 10

Electrons travel around the atom’s nucleus at incredibly fast speeds along imaginary tracks known as ___.

Answer 10

orbitals

Question 11

The ___ ___ is the standard table that organizes all known elements by atomic number; it is further organized into groups and periods that provide additional information about each element based on its relative position within the table.

Answer 11

Periodic Table

Question 12

What are the rows on the periodic table called?

Answer 12

Periods

Question 13

The area around the nucleus is called the ___ ___ because the electrons are rarely in one place for long.

Answer 13

electron cloud

Question 13

What are the columns on the periodic table called?

Answer 13

Groups

Question 14

Metals are on the ___ side of the periodic table, metalloids are in the ___, and nonmetals are on the ___.

Answer 14

left

middle

right

Question 15

What are found on the left side of the periodic table?

Answer 15

metals

Question 15

What dictates how reactive an element is?

Answer 15

number of electrons

Question 15

What are found in the middle of the periodic table?

Answer 15

metalloids

Question 16

What are found on the right side of the periodic table?

Answer 16

non-metals

Question 16

Atoms want to have a full outer electron shell. This means the atom needs 8 electrons in the outer orbital or shell. This is called the ___ rule.

Answer 16

octet rule

Question 16

The ___ (horizontal) on the periodic table are called periods, while the ___ (vertical) are called groups (also called families)

Answer 16

rows

columns

Question 17

How many electrons does an atom need on the outer shell to be “full?”

Answer 17

8 electrons

Question 18

The number of electrons in the ___ level of the electron cloud dictates how reactive an element is.

Answer 18

outer

Question 18

What is the octet rule?

Answer 18

Atoms want to have a full outer electron shell. This means the atom needs 8 electrons in the outer orbital or shell.

Question 19

Which group of atoms on the periodic table of elements is “fat and happy,” and has all 8 electrons on the outer shell?

Answer 19

Group 8

Question 19

An atom with a full outer shell will be ___ reactive because it does not need additional electrons to fill its outer shell

Answer 19

less

Question 20

An atom with a ___ outer shell will be less reactive because it does not need additional electrons to fill its outer shell – it is said to be ___. By less reactive, we mean that they are less likely to take or give away electrons to another atom because they already have ___ electrons in the outer shell.

Answer 20

full

stable

8

Question 21

An element with only 1 electron in its outer shell is unstable and highly ___, meaning it needs to bond with other atoms to fill its outer shell and become ____.

Answer 21

reactive

stable

Question 22

If electrons do not have 8 electrons, they tend to be ___ reactive, hoping to form a more stable compound where their outer shell has 8 electrons.

Answer 22

more

Question 23

Elements with ___ or ___ electrons in the outer shell are the most unstable and highly reactive.

Answer 23

1 or 7

Question 23

As you move from left to right across the periodic table by group, the elements become less reactive and, therefore, ___ likely to bond with other atoms or compounds (except for atoms in Group ___).

Answer 23

less

7

Question 24

Remember the octet rule! Atoms generally prefer to have ___ electrons in their outermost shell.

Answer 24

8

Question 24

This is the case for all the atoms in Group 8 (except He, which only has 2). Each of those elements (also known as the ___ gases) has a full outer shell of ___ electrons.

Answer 24

noble

8

Question 24

The elements in Group 8 are (less/more) reactive.

Answer 24

less

*they do not need additional electrons

Question 25

The ___ ___ is the number of protons plus neutrons in the nucleus of an atom. This number is usually located on the bottom or top right corner of an atom’s box on the periodic table.

Answer 25

atomic mass

Question 25

The ___ ___ is the number of protons in the nucleus of an atom, usually located in the top or top left corner of an atom’s box on the periodic table. This is always a whole number.

Answer 25

atomic number

Question 25

The ___ ___ is often and improperly used interchangeably with the term ‘atomic mass,’ this term actually represents the average weight of all a particular element’s isotopes. This value is NOT displayed on the periodic table.

Answer 25

atomic weight

Question 26

The atomic number of an element is also the number of ___ in each atom of that element.

Answer 26

protons

Question 27

For example, in Carbon (above), the atomic number is 6. This number represents the number of ___ in one atom of Carbon.

Answer 27

protons

Question 28

Therefore, the number of ___ in an atom defines that atom’s identity. This means that you can count the number of protons in an atom’s diagram and determine the atom’s ___.

Answer 28

protons

identity

Question 28

Atoms with a neutral charge will have an ___ number of electrons and protons. This is because each proton has a charge of ___, and each electron has a charge of ___.

Answer 28

equal

+1

-1

Question 28

Equal numbers of each mean they cancel out each other’s charges. Therefore, the atomic number is also equal to the number of ___ in the atom IF the atom is neutral.

Answer 28

electrons

Question 29

___ ___ is also known as the mass number of an element.

Answer 29

Atomic mass

Question 30

Atomic mass is the total mass of the particles in the nucleus – the mass of the ___ the mass of the ___.

Answer 30

protons

neutrons

Question 31

Electrons are ___ included in an atom’s mass because they are too ___ to have a significant contribution to the mass.

Answer 31

not

tiny

Question 31

What is not included in an atom’s mass?

Answer 31

electrons

Question 31

A proton is equal to one atomic mass unit. So, one proton is equal to “___” in the atomic mass value. A neutron is equal to 1.008 atomic mass units. Since it is so close to 1, we can also say that one neutron is equal to “___” in the atomic mass value.

Answer 31

1

1

Question 32

The atoms in the periodic table have an ___ number of protons and electrons.

Answer 32

equal

Question 33

Note that atomic mass is ___ the same as the atomic weight.

Answer 33

not

Question 33

Therefore, if an atom has an atomic mass of 2, it has ___ proton and ___ neutron. If it has an atomic mass of 4, it has ___ protons and ___ neutrons.

Answer 33

1,1

2,2

Question 33

An isotope has a different number of ___.

We find the number of neutrons by subtracting the number of protons from the ___ ___!

Answer 33

neutrons

atomic mass

Question 33

Isotypes have the same atomic number and number of ___ but a different number of ___.

Answer 33

protons

neutrons

Question 34

if we have an atom with a different number of neutrons, it will affect the atomic mass of that particular isotope. It will either be ___ or ___ than a “normal” atom of that element. It also means that the atomic mass of the isotope will be ___ from what’s included on the periodic table.

Answer 34

lighter

heavier

different

Question 34

When two atoms have the same number of protons but differ in their number of neutrons, what do we call this?

Answer 34

isotypes

Question 34

We know that Carbon has 6 protons because its atomic number is ___. To determine the number of neutrons in a single atom of Carbon, we can subtract 6 from 12, the atomic mass. Therefore, the number of its neutrons equals ___.

Answer 34

6

6

Question 35

An ___ is two or more versions of the same element and atom that have the same number of protons but differ in their number of neutrons.

Answer 35

isotope

Question 35

A positive Ion is also known as ___ and a negative ion is also known as an ___.

Answer 35

cation

anion

Question 36

In the case of Phosphorus-25, we would subtract Phosphorus’s atomic number (15) from the isotope’s atomic mass (25).

25 – 15 = 10 → This means that there are ___ neutrons in this isotope of Phosphorus. Phosphorus-25 has 5 less neutrons than a “normal” atom of Phosphorus.

Answer 36

10

Question 36

What is a cation?

Answer 36

a positive ion

Question 36

A ___ ___ is a version of a particular atom that has more electrons that protons – it is also called an anion.

Answer 36

Negative Ion

Question 37

A ___ ___ is a version of a particular atom that has more protons than electrons – it is also called a cation

Answer 37

positive ion

Question 37

You’ll know an isotope when you see it because of how the name is written.

25P or Phosphorus-25 is an isotope. The 25 represents the ATOMIC ___ of the isotope, NOT the number of neutrons.

Answer 37

MASS

Question 38

What is an anion?

Answer 38

a negative ion

Question 39

An ___ ___ is a bond that occurs when atoms with opposite charges share or transfer electrons to one another.

Answer 39

ionic bond

Question 39

Ionization occurs when atoms with ___ charge are turned into atoms with ___ or ___ charges.

Answer 39

no

positive

negative

Question 39

When atoms with opposite charges share or transfer electrons to one another, what kind of bond do we call this?

Answer 39

ionic bond

Question 39

Atoms and molecules are generally neutral (having no charge), meaning the positive charge of the protons in the nucleus is balanced by the negative charge of surrounding electrons.

Answer 39

neutral

Question 39

Sometimes the number of protons and electrons are ___ equal. When that is the case, the atom will carry an electrical charge.

Answer 39

not

Question 39

When the number of protons and electrons are not equal, the atom will carry an ___ charge.

Answer 39

electrical

Question 40

___ is the process through which neutral (no charge) atoms are turned into atoms with positive or negative charges.

Answer 40

Ionzation

Question 40

If the atom has more electrons than protons, then it will have a ___ charge.

Answer 40

negative

Question 40

Protons carry a ___ charge (+1), electrons carry a ___ charge (-1), and neutrons do ___ have a charge

Answer 40

positive

negative

not

Question 40

___ is the process of an atom or molecule acquiring a positive or negative charge by losing or gaining an electron.

Answer 40

Ionization

Question 40

If the atom has more protons than electrons, then it will have a ___ charge.

Answer 40

positive

Question 41

Remember that electrons carry a negative charge. So, if an atom loses an electron, it loses a ___ charge. When it loses an electron, it now has one more proton than electrons, so it would have a (+1) overall ___ charge.

Answer 41

negative

positive

Question 42

If an atom gains an electron, it adds another ___ charge. This means the atom has one more electron than protons, so it would have a ___ overall charge.

Answer 42

negative

negative

Question 42

One of the most common ionic compounds we are familiar with is sodium chloride, or as we know it, table salt. Sodium tends to exist as a ___ ion and chlorine typically exists as a ___ ion. When in close proximity, they bond together (like magnets) and the resulting compound has a ___ (zero) charge.

Answer 42

positive

negative

neutral

Question 43

Ionic bonds are like magnets. Every magnet has a ___ and a ___ side. When the positive and negative sides get near to one another, the magnets pull toward each other to connect. When in close proximity, ions bond together (like magnets) and the resulting compound has a neutral (___) charge.

Answer 43

positive

negative

zero

Question 43

The ___ ___ is an imaginary track or orbital on which electrons travel around the nucleus of an atom.

Answer 43

electron shell

Question 44

The ___ ___ is any electron traveling on the valence shell of an atom.

Answer 44

valence electron

Question 44

The ___ ___ is the outermost electron shell surrounding the nucleus of an atom

Answer 44

valence shell

Question 45

Electrons travel around the nucleus of the atom at incredibly fast speeds along imaginary tracks called orbitals called ___ ___.

Answer 45

electron shells

Question 46

Each of the orbitals in an atom can hold a ___ number of electrons.

Answer 46

specific

Question 47

Each level must be ___ before a new level is added.

When the outermost shell of an electron contains the maximum number of electrons it can hold, the atom is considered ___.

Answer 47

filled

stable

Question 47

The first orbital or shell can hold ___ electrons; the second orbital can hold ___ electrons; the third orbital can hold ___ electrons; the fourth orbital can hold ___ electrons.

Answer 47

2

8

18

32

Question 48

Recall that a neutral atom of an element will have an equal number of protons and electrons. We know the atomic number of Mg is 12. This means there are 12 protons. Assuming an atom of Mg is neutral, how many electrons will it have?

Answer 48

12 electrons

Question 49

The first orbital will contain its maximum number of electrons which is ___ electrons. This leaves 10 more electrons that need a home. The next shell, the 2nd orbital, can hold ___ electrons. Therefore, 8 of the remaining 10 electrons will exist on the second orbital of Mg. There are 2 left! The last 2 electrons will exist on the third orbital. This means that a neutral atom of Mg has __ valence electrons.

Answer 49

2

8

2

Question 50

The electrons in the valence shell are called ___ ___.

Answer 50

valence electrons

Question 50

If the outermost shell, or valence shell, is not full, then the atom will be ___ likely to bond with other atoms.

The atom will attempt to bond so that the valence shell becomes ___.

Answer 50

more

full

Question 51

What dictates the bonding behavior of the atom?

Answer 51

electrons

Question 52

___ are a group of atoms that are bonded together; they are the smallest unit of matter that can participate in chemical reactions.

Answer 52

Molecules

Question 53

___ are formed when one or more atoms bind together.

Answer 53

Compounds

Question 54

___ ___ is atomic bonding that occurs when atoms share valence electrons

Answer 54

Covalent bonding

Question 54

___ ___ is atomic bonding due to electrostatic attraction between two oppositely charged ions

Answer 54

Ionic bonding

Question 55

___ ___ is atomic or molecular bonding that occurs when an atom or molecule bonds to a hydrogen atom within the same or a different compound or molecule

Answer 55

Hydrogen bonding

Question 56

A positively charged ion is called a ___.

Answer 56

cation

Question 57

A negatively charged ion is called an ___.

Answer 57

anion

Question 58

What is the degree of how capable an atom is of attracting the electrons of another atom?

Answer 58

electronegativity

Question 58

A ___ bond (___ covalent bond) occurs when atoms that engage in bonding have a small difference in electrical charges.

Answer 58

polar

polar

Question 59

A ___ bond (pure ___ covalent bond) occurs when there is no electronegativity.

Answer 59

nonpolar

nonpolar

Question 60

A ___ is a pair of oppositely charged ions that form a bond

Answer 60

Dipole

Question 60

When atoms bind together, they form a ___.

Answer 60

compound

Question 61

Compounds form larger particles called ___.

Answer 61

molecules

Question 62

A molecule is a ___ of atoms that are bonded together.

Answer 62

group

Question 63

A molecule’s bonding behavior is affected by the ___ of the compounds and the physical structure of the molecules (including the atoms they consist of).

Answer 63

properties

Question 63

Chemical bonding occurs when ___ are shared with, given to, or taken away from another atom.

Answer 63

electrons

Question 64

Ionic bonding happens specifically between two ___ charged ions.

Answer 64

oppositely

Question 64

What are the three main types of bonding?

Answer 64

ionic bonding

covalent bonding

hydrogen bonding

Question 64

There are three main types of chemical bonding: ___ bonding, ___ bonding, and ___ bonding.

Answer 64

ionic

covalent

hydrogen

Question 64

Remember that ions are charged atoms with ___ or ___ electrons than protons (never equal).

Answer 64

more

fewer

Question 65

What type of bonding occurs when an atom gains or loses electrons and becomes either positively or negatively charged as a result?

Answer 65

ionic bonding

Question 66

In ionic bonding, atoms gain or lose ___ and become positively or negatively charged as a result.

Answer 66

electrons

Question 66

An ionic bond exists when two oppositely ___ ions are bonded due to the electrostatic attraction between the two.

Answer 66

charged

Question 66

Ionic bonds are most common between which two materials?

Answer 66

metal and nonmetals

Question 67

___ ___ occurs when atoms share valence electrons between them to complete both of their outer shells.

Answer 67

Covalent bonding

Question 67

What do atoms share when they have a covalent bond to complete both of their outer shells?

Answer 67

valence electrons

Question 68

Nonmetals tend to engage in ___ bonds with each other, while bonds between metals and nonmetals are typically ___ in nature.

Answer 68

covalent

ionic

Question 69

Which kind of elements engage in covalent bonds with each other? Which kind of elements engage in ionic bonds with each other?

Answer 69

nonmetals

metals with nonmetals

Question 70

When valence electrons are shared equally between atoms, they are said to have a ___ bond.

Answer 70

nonpolar

Question 70

What are the two primary types of covalent bonds?

Answer 70

polar covalent bonds

nonpolar covalent bonds

Question 70

If electrons are shared equally, there is ___ difference in the electronegativity of the atoms involved in bonding. This occurs in ___ bonds.

Answer 70

no

nonpolar

Question 70

In covalent bonding, the electrons are shared in order for all the atoms involved in the bond to have ___ shells.

Answer 70

full

Question 70

Why do atoms engage in covalent bonding?

Answer 70

the electrons are shared in order for all the atoms involved in the bond to have full shells

Question 71

Electrons that are shared unequally have a stronger electrical pull on the electrons. This occurs in ___ bonds.

Answer 71

polar

Question 71

When electrons are shared unequally, they are said to have a ___ bond.

Answer 71

polar

Question 72

A polar covalent bond occurs when there is a ___ difference in electronegativity.

Contrast this with an ionic bond where the difference in electronegativity between the atoms is ___ (for example, one atom with 1 valence electron bonding with another with 7 valence electrons).

Answer 72

small

larger

Question 73

___ ___ occurs when an atom within molecule bonds with a hydrogen atom.

Answer 73

Hydrogen bonding

Question 74

H2O is a ___ covalent molecule – the electrons are slightly closer to the oxygen atom.

Answer 74

polar

Question 74

One of the most common places we see hydrogen bonding is between ___ molecules.

Answer 74

water

Question 75

Water’s polar covalent bonding gives oxygen a slight ___ charge, while hydrogen then ends up with a slightly ___ charge. The opposite charges attract, and the water molecules are bound together with hydrogen bonds.

Answer 75

negative

positive

Question 76

The hydrogen bound to oxygen in a single H2O (water) molecule, is a polar covalent bond, ___ a hydrogen bond. However, the hydrogen atom of one H2O molecule bonded to the oxygen atom of another H2O is considered a ___ bond.

Answer 76

not

hydrogen

Question 76

A ___ ___ is a chemical combination of two or more elements.

Answer 76

chemical compound

Question 76

How many bonds do alkanes have between their carbon atoms?

Answer 76

one (single bonds)

Question 77

___ are organic compounds that have only a single bond between their carbon atoms.

Answer 77

Alkanes

Question 77

___ are organic compounds that have at least one double bond between their carbon atoms.

Answer 77

Alkenes

Question 78

___ are organic compounds that have at least one triple bond between their carbon atoms.

Answer 78

Alkynes

Question 78

How many bonds do alkynes have between their carbon atoms?

Answer 78

3 (triple bonds)

Question 79

There are several compounds that are only composed of hydrogen and carbon. The compounds that only consist of hydrogen and carbon are called ___ ___.

Answer 79

organic compounds

Question 79

Alkanes have only a ___ bond between their carbon atoms.

Answer 79

single

Question 79

What are the three types of hydrocarbons?

Answer 79

alkanes

alkenes

alkynes

Question 80

How many bonds do alkenes have between their carbon atoms?

Answer 80

2 (double bonds)

Question 80

A ___ is made up of chemically bonded atoms of individual elements.

Answer 80

compound

Question 80

Methane (CH4), Ethane (C2H6), Propane (C3H8), and Butane (C4H10) are examples of ___.

Answer 80

alkanes

Question 81

As you may have noticed, the suffix of the alkanes all end in “___”.

Answer 81

“ane”

Question 81

Alkenes have at least one ___ bond between one set of carbon atoms.

Answer 81

double

Question 81

Ethene (C2H4), Propene, 1-Butene, 2-pentene are examples of ____.

Answer 81

alkenes

Question 81

Alkynes have at least one ___ bond between two of their carbon atoms.

Answer 81

triple

Question 82

As you may have noticed, the suffix of the alkenes all end in “___”.

Answer 82

“-ene”

Question 83

Ethyne, 1-propyne, 1-butyne, 1-pentyne arre examples of ___.

Answer 83

alkynes

Question 84

Note, the suffix of the alkynes all end in “___”.

Answer 84

“-yne”

Question 85

Hydrocarbons with a single bond are known as ___.

Answer 85

alkanes

Question 85

Hydrocarbons with a triple bond are known as ___.

Answer 85

alkynes

Question 86

Hydrocarbons with a double bond are known as ___.

Answer 86

alkenes

Question 86

Hydrocarbons are organic compounds made up of only ___ (H) and ___ (C).

Answer 86

hydrogens

carbons

Question 87

What do call the set of words placed before the hydrocarbon’s name that indicates the number of carbons in the main chain of the hydrocarbon’s structure?

Answer 87

hydrocarbon prefixes

Question 88

___ are hydrocarbons that contain only single bonds.

Answer 88

Alkanes

Question 88

___ are hydrocarbons that contain at least one double bond.

Answer 88

Alkenes

Question 89

___ are hydrocarbons that contain at least one triple bond.

Answer 89

Alkynes

Question 90

The name of a hydrocarbon depends on the number of ___ that it has in its main chain.

Answer 90

carbons

Question 91

The first step of the process of naming a hydrocarbon is to identify the ___ chain in its structure and then count the number of carbons it has. The prefix that will be used depends on the number of ___.

Answer 91

longest

carbons

Question 91

How many carbons does the prefix Meth- signify?

Answer 91

1

Question 92

How many carbons does the prefix Eth- signify?

Answer 92

2

Question 92

How many carbons does the prefix Prop- signify?

Answer 92

3

Question 93

How many carbons does the prefix But- signify?

Answer 93

4

Question 94

How many carbons does the prefix Penta- signify?

Answer 94

5

Question 94

How many carbons does the prefix Hexa- signify?

Answer 94

6

Question 95

How many carbons does the prefix Hepta- signify?

Answer 95

7

Question 95

How many carbons does the prefix Octa- signify?

Answer 95

8

Question 96

How many carbons does the prefix Nona- signify?

Answer 96

9

Question 96

How many carbons does the prefix Deca- signify?

Answer 96

10

Question 97

Then, the ___ that will be given to the hydrocarbon depends on whether it is an alkane, an alkene, or an alkyne,

Answer 97

suffix

Question 98

What suffix do hydrocarbons have that are alkanes?

Answer 98

-ane

Question 99

What suffix do hydrocarbons have that are alkenes?

Answer 99

-ene

Question 99

What suffix do hydrocarbons have that are alkynes?

Answer 99

-yne

Question 99

When naming hydrocarbons, the first step would be to identify the ___ chain in the structure.

Then the next step is to count the number of ___ atoms in the main chain.

If the number of carbons is equal to 3, the prefix to be used is prop-. If the number of carbons is equal to 7, the prefix to be used is ___.

To finish the name, we give a suffix according to the type of hydrocarbon, what kind of bonds there are.

If the hydrocarbon has a triple bond, it is an alkyne, so the suffix will be ___.

Answer 99

longest

carbon

hepta-

-yne

Question 99

For alkenes and alkynes, the ___ of the double or triple bond needs to be included in the name of the structure.

For example, the name of the molecule in the image is 2-butene, because the ___bond is located on the number 2 carbon atom counting from the end closest to the double bond

Answer 99

position

double

Question 100

Which organic compounds contain the hydroxyl group (-OH) bonded to a saturated carbon atom?

Answer 100

Alcohols

Question 101

What is the general formula for alcohols?

Answer 101

R-OH

Question 102

___ have the general formula R-OH, where R is an alkyl group.

Answer 102

Alcohols

Question 102

Alcohols are named by adding the suffix “___” after the prefix of the main alkyl chain.

Answer 102

“-ol”

Question 103

For alcohols with more than ___ carbon atoms, the position of the -OH group must be indicated with a location number that is found by counting from the end of the molecule closer to the hydroxyl group.

This means that the alcohol CH3CH2CH2OH is called ___.

Answer 103

2

1-propanol
(“prop-” + “-ane-” + “-ol”)

Question 103

To recognize an alcohol, just look for the “___” group!

Answer 103

“-OH”

Question 103

What is the structure of methanol?

Answer 103

CH3OH

*The structure of methanol is an alcohol in which R is a methyl group ( −CH3 )

Question 104

___ are organic compounds that contain two alkyl groups linked by an oxygen atom.

Answer 104

Ethers

Question 105

An ___ ___ is a radical that is formed by removing a hydrogen atom from an alkane chain.

Answer 105

alkyl group

Question 105

___ have the general formula ROR’.

Answer 105

Ethers

Question 106

Ethers have the general formula ___, where R and R’ are alkyl groups

Answer 106

ROR’

Question 106

How many ways are there to name ethers?

Answer 106

2

Question 107

The first way to name an ether is to identify the length of the R and R’ groups. The ___ group becomes the base chain (named following the rules for hydrocarbons) and the ___ group becomes the alkoxy substituent.

For example, in the ether CH3OCH2CH3 , the −CH2CH3 group is the longer R group, so it becomes the base. The base name is ___. The shorter R’ group is the CH3, so the CH3O− group is the ___ substituent (methoxy). The complete name of CH3OCH2CH3 is methoxy ethane.

Answer 107

longer

shorter

ethane

alkoxy

Question 107

The second way of naming ethers is by naming the R and R’ groups ___ (prefix + “yl”) in alphabetical order, followed by the word “ether”.

For example, in the ether CH3CH2OCH2CH2CH3 , the names of the R and R’ groups are ___ (for the CH3CH2- group) and ___ (for the −CH2CH2CH3 group), so the name of this ether would be ethyl propyl ether.

If the two groups are the same, then the R group is named only once, with the prefix “di-” before its name (e.g. CH3OCH3 would be ___ ___).

Answer 107

separately

ethyl

propyl

dimethyl ether

Question 108

To recognize an ether, just look for the ___ group!

Answer 108

C-O-C

Question 108

Be careful – if the C-O-C group is next to a carbonyl (C=O) group, then the molecule is NOT an ether but an ___.

Answer 108

ester

Question 109

An ___ is an organic compound that contains a carbonyl group bonded to an alkyl group and a hydrogen atom.

Answer 109

Aldehyde

Question 109

An ___ group is a radical that is formed by removing a hydrogen atom from an alkane chain.

Answer 109

alkyl

Question 109

A ___ group is a functional group that contains a carbon atom forming a double bond with an oxygen atom (C=O).

Answer 109

carbonyl

Question 110

___ have the general formula RCHO (it is not written RCOH to avoid confusing an aldehyde with an alcohol).

Answer 110

Aldehydes

Question 111

Aldehydes have the general formula ___.

Answer 111

RCHO

Question 112

Aldehydes are named by using the prefix of the parent alkane chain and adding the suffix “___”.

For example, the aldehyde CH3CHO would be named “___”.

Answer 112

“-al”

ethanal

Question 113

Another usual way of naming aldehydes is by using the common name of the parent chain and adding the suffix “___” at the end.

The simplest aldehyde, formaldehyde (HCHO), does not have an R group.

Answer 113

“-aldehyde”

Question 114

An ___ is an organic compound that contains a carbonyl group (C=O) bonded to an alkyl group (-R) and a hydrogen atom (-H).

Answer 114

aldehyde

Question 115

A ___ group is a functional group that contains a carbon atom forming a double bond with an oxygen atom (C=O).

Answer 115

carbonyl

Question 116

___ have the general formula RCOR’ (CO is the carbonyl group, C=O).

Answer 116

Ketones

Question 117

Ketones have the general formula ___ (CO is the carbonyl group, C=O).

Answer 117

RCOR’

Question 117

For ketones with 5 or more carbon atoms, the position of the carbonyl group needs to be indicated with a location number that is found by counting from the end of the molecule ___ to the carbonyl group.

For example, the ketone CH3CH2CH2COCH3 would be named ___ (since the carbonyl group is closer to the right of the molecule, carbon atoms are counted from right to left).

Answer 117

closer

2-pentanone

Question 117

Ketones are named by using the prefix of the parent alkane chain and adding the suffix “___” at the end.

Answer 117

“-one”

Question 118

Another way of naming ketones is by naming the R and R’ groups ___ (with the prefix that indicates the length of the carbon chain and the suffix “-yl”) in alphabetical order, followed by the word “ketone”.

This means that the ketone CH3CH2CH2COCH3 can also be named methyl propyl ketone.

Answer 118

separately

Question 119

If the R and R’ groups are equal (which means the ketone is symmetrical), then the prefix “___” is added before the name of the R group, which is named only once. This means that the ketone CH3CH2COCH2CH3 can be named 3-pentanone or diethyl ketone.

Answer 119

“di-“

Question 119

What is the simplest and most common ketone?

Answer 119

acetone

Question 119

Ketones and aldehydes are very similar, but ___ have a hydrogen atom bonded to the carbonyl group, and ___ have two alkyl groups bonded to the carbonyl group.

Answer 119

aldehydes

ketones

Question 120

___ ___ are organic compounds that contain a carbonyl group (C=O) bonded to an alkyl group (-R) and a hydroxyl group (-OH).

Answer 120

Carboxylic acid

Question 120

Carboxylic acids have the general formula ___ (CO is the carbonyl group, C=O).

Answer 120

RCOOH

Question 120

___ ___ have the general formula RCOOH (CO is the carbonyl group, C=O).

Answer 120

Carboxylic acids

Question 121

The ___ group is also known as the carboxylate group.

Answer 121

-COOH

Question 122

Carboxylic acids are named by using the prefix of the parent alkane chain and adding the suffix “___ ___” at the end

Answer 122

“-anoic acid”

Question 123

For example, the carboxylic acid CH3CH2CH2COOH would be named ___ ___.

Answer 123

butanoic acid

Question 124

What are the two classes of carboxylic acids with great biological importance?

Answer 124

fatty acids

amino acids

Question 125

___ ___ are carboxylic acids that usually have between 12 and 20 carbon atoms in their R group. They can be ___ if they contain double bonds or ___ if they only contain single bonds.

Answer 125

Fatty acids

unsaturated

saturated

Question 125

An ___ is a hydrocarbon that contains at least one double bond and has the general formula CnH2n.

Answer 125

Alkene

Question 126

A ___ is an organic aromatic cyclic compound with molecular formula C6H6.

Answer 126

Benzene

Question 127

A ___ is an organic compound that contains 3 or more alternating double and single bonds.

Answer 127

Polyene

Question 128

___ is a planar ring with 6 carbon atoms with equal C-C bond length. Each of the carbons is bonded to a hydrogen atom.

Answer 128

Benzene

Question 129

Benzene is a planar ring with ___ carbon atoms with equal C-C bond length. Each of the carbons is bonded to a hydrogen atom.

Answer 129

6

Question 130

The special structure of benzene is responsible for many of its unique properties. For example, it is fairly ___ towards reactions.

The delocalized electrons in benzene are not easily available to react, and that gives benzene great ___.

Answer 130

unreactive

stability

Question 131

___ are organic compounds that contain the amine group (−NH2).

Answer 131

Amines

Question 132

Amines are organic compounds that contain the amine group (___).

Answer 132

−NH2

Question 133

Up to ___ alkyl groups may be bonded to the nitrogen atom, replacing the hydrogen atoms in ammonia. The nitrogen atom in amines has a lone pair of electrons

Answer 133

3

Question 134

Amines are named using the word “___” as a substitute on the main chain.

For example, the amine CH3CH2CH2NH2 would be named ___.

Answer 134

“amino-“

1-aminopropane

Question 135

Amines show ___ behavior, which means they’re able to donate an electron pair or accept a proton from an acid.

Answer 135

basic

Question 135

Another way of naming amines is by using the suffix “___” after the prefix for the main alkyl chain, and for 2° and 3° amines, the substituents on the nitrogen atom are indicated by the prefix “N-” before the name of the alkyl group.

This means the amine CH3N(CH3)2 can also be named N,N-dimethylmethanamine.

Answer 135

“-amine”

Question 136

As there are more alkyl groups bonded to the nitrogen atom, and as they are longer, the amine is ___ basic, due to the increased electron density.

Answer 136

more

Question 137

Which of the following atoms has the largest atomic radius?

Mg
Be
Ra
Sr

Answer 137

Ra

*The atomic radius increases as you move down a group (column) in the periodic table. Atoms further down a group (closer to the bottom) have more electron shells.

Question 138

How many neutrons does an atom of Gd have?

Answer 138

93

*The number of neutrons of an atom is equal to the atom’s mass number minus the number of protons (atomic mass – atomic number = number of neutrons).

Question 139

Which of the following has 35 protons, 45 neutrons, and 36 electrons?

Rh3+
Br–
P3-
Kr

Answer 139

Br-

Question 140

How many electrons does a sodium ion (Na+) have?

Answer 140

10

Question 140

How many valence electrons does sodium have?

Answer 140

1

Question 141

How many valence electrons does the sulfide ion S2- have?

Answer 141

8

Question 142

Which of the following atoms will form an ion that is larger than the neutral atom?

Na+
Al3+
Mg2+
Cl–

Answer 142

Cl-

*Cations are always smaller than neutral atoms because they have lost one or more electrons (e.g., Na+, Mg2+, and Al3+ are smaller than Na, Mg, and Al, respectively).

In contrast, anions are always larger than the neutral atom because they have gained an electron (e.g., Cl– is larger than Cl).

Question 143

What is the difference between rubidium-87 and rubidium-82?

Answer 143

Rubidium-87 has 5 more neutrons than rubidium-82.

*Rubidium-87 and rubidium-82 are isotopes of rubidium, meaning that they have the same number of protons and electrons, but different numbers of neutrons.

Question 143

What is the charge on a sulfide ion?

Answer 143

2-

*Sulfur belongs to group 6A of the periodic table. This means that it needs to gain two electrons to have a full octet. When it gains two electrons, it gains two more negative charges as compared to the neutral sulfur atom, giving the sulfide ion (S2-) a 2- charge.

Question 144

Which of the following represent isotopes of the same element?

Fe2+ and Fe3+
55Fe and 56Fe
H– and H+
Cl and Cl–

Answer 144

55Fe and 56Fe

*The superscripts to the left of Fe in option B represent the mass numbers (the sum of protons and neutrons) of the respective iron atoms. 55Fe and 56Fe represent different isotopes of Fe because they have the same number of protons (26), but different numbers of neutrons.

Question 145

What is the charge on a nitride ion?

Answer 145

3-

*Nitrogen belongs to group 5A of the periodic table. This means that it needs to gain three valence electrons in order to have a full octet. By gaining three electrons, it gains three extra negative charges, thus giving the nitride ion (N3-) a 3- charge.

Question 146

What charge will an ion of chlorine-37 have?

Answer 146

-1

*ISOTOPES are atoms that have the same number of protons, but a different number of neutrons. For example, both chlorine-35 and chlorine-37 have 17 protons, but chlorine-37 has two extra neutrons and a total of 20 neutrons.
IONS are charged atoms that have an excess number of either protons (positively-charged cations) or electrons (negatively-charged anions). Chlorine-37 contains 17 protons, so it also contains 17 electrons (7 of which are valence electrons); therefore, it gains one electron to obtain a full octet, thus taking on a -1 charge.

Question 146

Which of the following are true of uranium-235?

select all that apply

• It has 235 neutrons.
• It has 235 electrons.
• It has 235 protons.
• It has 143 electrons.
• It has 143 neutrons.
• It has 92 protons.

Answer 146

• It has 143 neutrons.
• It has 92 protons.

*The number 235 indicates the mass number of the given Uranium isotope, which is the sum of the number of its protons and neutrons. Uranium has an atomic number of 92. Accordingly, a uranium-235 atom has 143 neutrons.

Question 146

Which of the following subshells can hold a maximum of 6 electrons?

Answer 146

p-subshell

*s subshells: Can hold a maximum of 2 electrons
p subshells: Can hold a maximum of 6 electrons
d subshells: Can hold a maximum of 10 electrons
f subshells: Can hold a maximum of 14 electrons

Question 147

Which of the following is true of oxygen-18?

It forms an ion with a -3 charge.
It has 8 protons.
It has 10 protons.
It has 10 electrons.

Answer 147

It has 8 protons.

Question 148

A neutral chlorine atom (Cl) has 7 electrons in its valence shell. Which of the following ions will it form?

Answer 148

Cl–

*A neutral chlorine atom has 7 valence electrons, so it needs to gain 1 more electron to have a complete octet. When it gains an electron, the chlorine atom has one more negatively-charged electron than positively-charged protons. So, the resulting ion has a -1 charge.

Question 148

Which of the subshells given below can hold additional electrons?

6f14
4d6
3p6
2s2

Answer 148

4d6

*s subshells: Can hold a maximum of 2 electrons
p subshells: Can hold a maximum of 6 electrons
d subshells: Can hold a maximum of 10 electrons
f subshells: Can hold a maximum of 14 electron

Question 148

Which of the given electron subshells needs an additional 2 electrons to have all of its orbitals completely filled?

4p3
5d6
6f12
4s1

Answer 148

6f12

*s subshells: Can hold a maximum of 2 electrons
p subshells: Can hold a maximum of 6 electrons
d subshells: Can hold a maximum of 10 electrons
f subshells: Can hold a maximum of 14 electron

Question 149

The electron configurations of several atoms are listed below. Which of them is most likely to lose electrons?

1s22s22p63s23p6
1s22s22p63s2
1s22s22p4
1s22s2

Answer 149

1s22s22p63s2

*Atoms form ions so that they can gain a complete octet of valence electrons.

1s22s22p4 would prefer to gain 2 electrons to obtain a complete octet.

1s22s22p63s23p6 already has a full octet.

Although options 1s22s2 and 1s22s22p63s2 have similar electron configurations, with 2 valence electrons in their s-orbitals, the electrons in the 3s orbital are easier to remove because they are farther from the nucleus. The electrons in the lower-lying subshells (1s,2s,2p) shield these valence electrons from the electrostatic attraction of protons in the nucleus. This makes it easier for them to be removed in order to form an ion.

Question 150

Which of the following represents the electron configuration of Li in LiCl?

Answer 150

1s2

Question 151

In which of the following types of bonds are valence electrons completely donated from one atom to the other?

Answer 151

Ionic bond

*Ionic bonding is the complete transfer of valence electron(s) between atoms.

In an ionic bond, the less electronegative atom donates its valence electrons to another, more electronegative atom. The atom that donates its electrons becomes a positively-charged cation, while the atom that accepts the electrons becomes a negatively-charged anion.

In covalent bonds, electrons are shared between two atoms.

Question 152

In which of the following bonds are electrons donated from one atom to another?

Answer 152

ionic bond

*In an ionic bond, the less electronegative atom donates its valence electrons to another, more electronegative atom. The atom that donates its electrons becomes a positively-charged cation, while the atom that accepts the electrons becomes a negatively-charged anion.

Question 153

Which of the compounds below contains both ionic and covalent bonds?

CO2
KOH
CH4
NaCl

Answer 153

KOH

*KOH contains both types of bonds: an ionic bond between the potassium ion K+ and hydroxide ion OH–, as well as a polar covalent bond between O and H.

Question 154

Which of the following properties mainly determines a bond’s polarity?

Answer 154

electronegativity

*electronegativity describes an atom’s ability to attract electrons; atoms with a higher electronegativity pull electrons towards them more strongly. An atom’s ability to attract electrons determines its polarity.

Question 155

Which of the following bonds do you expect to be the most polar?

H-H
C-C
C-F
C-O

Answer 155

C-F

*The bond with the largest electronegativity difference is the most polar

Question 156

Which of the following bonds do you expect to be nonpolar?

Answer 156

C-C

*The atoms in C-C are identical, so they have the same polarity; therefore, they form nonpolar covalent bonds (electrons are shared equally). In the other options, the electrons are shared unequally between the respective atoms due to the difference in their electronegativities, thus making them polar covalent bonds.

Question 157

Which of the atom pairs below would form an ionic bond with each other?

N and O
He and Ar
C and H
Mg and O

Answer 157

Mg and O

Question 158

Which of the following atoms would oxygen (O) form an ionic bond with?

Na
O
S
N

Answer 158

Na

Question 159

Which of the following has the longest bond length?

C-I
C-Br
C-Cl
C-F

Answer 159

*Non-polar bonds are generally longer than polar bonds

Larger atoms have longer bonds

Single bonds are longer than double or triple bonds

The bond length between two atoms is the distance between their nuclei. The distance increases as the size of the atoms increases. We know from periodic trends that the size of atoms in the same group increases as we move down a group (column). Iodine (I) is the lowermost atom in the halogen group of the periodic table. Therefore, it will form the longest bond with carbon.

Question 160

Which of the following will have the shortest bond length?

All bonds are the same length.
C≡N
C=N
C-N

Answer 160

C≡N

*Single bonds are longer than double or triple bonds

As the bond order (the number of electron bonding pairs) increases between two atoms, the distance between the two atoms decreases. This means as more bonds are formed between two atoms, they move closer to each other. Consequently, the bond length decreases.