TEAS 7 - Science (Atomic Structure) Flashcards
An ____ is the smallest unit of matter.
atom
The ___ is the center of the atom, which is made up of protons and neutrons
nucleus
What are the two numbers that make up the atomic mass?
protons and neutrons
A ___is a neutrally charged subatomic particle; it is located in the nucleus at the center of the atom
neutron
The atomic number of elements on the Periodic Table of Elements is the element’s ___ ___.
atomic number
An ___ is a negatively charged subatomic particle that moves around the outside of the nucleus of an atom along circular paths called orbitals.
electron
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
proton
What is the smallest unit of matter?
atoms
___ 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
Orbitals
What is the charge of a proton? Neutron? Electron?
Proton: (+)
Neutron: none
Electron: (-)
The ___ ___ is the area around the nucleus of an atom that contains electrons traveling around the nucleus.
electron cloud
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.”
nucleus
protons
neutrons
electrons
The ___ is located at the center of an atom.
nucleus
What is the nucleus made of?
protons and neutrons
___ have a positive charge.
___ have a neutral charge.
___ have a negative electrical charge.
Protons
Neutrons
Electrons
What obits the nucleus in rings?
electrons
Electrons travel around the atom’s nucleus at incredibly fast speeds along imaginary tracks known as ___.
orbitals
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.
Periodic Table
What are the rows on the periodic table called?
Periods
The area around the nucleus is called the ___ ___ because the electrons are rarely in one place for long.
electron cloud
What are the columns on the periodic table called?
Groups
Metals are on the ___ side of the periodic table, metalloids are in the ___, and nonmetals are on the ___.
left
middle
right
What are found on the left side of the periodic table?
metals
What dictates how reactive an element is?
number of electrons
What are found in the middle of the periodic table?
metalloids
What are found on the right side of the periodic table?
non-metals
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.
octet rule
The ___ (horizontal) on the periodic table are called periods, while the ___ (vertical) are called groups (also called families)
rows
columns
How many electrons does an atom need on the outer shell to be “full?”
8 electrons
The number of electrons in the ___ level of the electron cloud dictates how reactive an element is.
outer
What is the octet rule?
Atoms want to have a full outer electron shell. This means the atom needs 8 electrons in the outer orbital or shell.
Which group of atoms on the periodic table of elements is “fat and happy,” and has all 8 electrons on the outer shell?
Group 8
An atom with a full outer shell will be ___ reactive because it does not need additional electrons to fill its outer shell
less
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.
full
stable
8
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 ____.
reactive
stable
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.
more
Elements with ___ or ___ electrons in the outer shell are the most unstable and highly reactive.
1 or 7
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 ___).
less
7
Remember the octet rule! Atoms generally prefer to have ___ electrons in their outermost shell.
8
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.
noble
8
The elements in Group 8 are (less/more) reactive.
less
*they do not need additional electrons
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.
atomic mass
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.
atomic number
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.
atomic weight
The atomic number of an element is also the number of ___ in each atom of that element.
protons
For example, in Carbon (above), the atomic number is 6. This number represents the number of ___ in one atom of Carbon.
protons
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 ___.
protons
identity
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 ___.
equal
+1
-1
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.
electrons
___ ___ is also known as the mass number of an element.
Atomic mass
Atomic mass is the total mass of the particles in the nucleus – the mass of the ___ the mass of the ___.
protons
neutrons
Electrons are ___ included in an atom’s mass because they are too ___ to have a significant contribution to the mass.
not
tiny
What is not included in an atom’s mass?
electrons
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.
1
1
The atoms in the periodic table have an ___ number of protons and electrons.
equal
Note that atomic mass is ___ the same as the atomic weight.
not
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.
1,1
2,2
An isotope has a different number of ___.
We find the number of neutrons by subtracting the number of protons from the ___ ___!
neutrons
atomic mass
Isotypes have the same atomic number and number of ___ but a different number of ___.
protons
neutrons
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.
lighter
heavier
different
When two atoms have the same number of protons but differ in their number of neutrons, what do we call this?
isotypes
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 ___.
6
6
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.
isotope
A positive Ion is also known as ___ and a negative ion is also known as an ___.
cation
anion
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.
10
What is a cation?
a positive ion
A ___ ___ is a version of a particular atom that has more electrons that protons – it is also called an anion.
Negative Ion
A ___ ___ is a version of a particular atom that has more protons than electrons – it is also called a cation
positive ion
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.
MASS
What is an anion?
a negative ion
An ___ ___ is a bond that occurs when atoms with opposite charges share or transfer electrons to one another.
ionic bond
Ionization occurs when atoms with ___ charge are turned into atoms with ___ or ___ charges.
no
positive
negative
When atoms with opposite charges share or transfer electrons to one another, what kind of bond do we call this?
ionic bond
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.
neutral
Sometimes the number of protons and electrons are ___ equal. When that is the case, the atom will carry an electrical charge.
not
When the number of protons and electrons are not equal, the atom will carry an ___ charge.
electrical
___ is the process through which neutral (no charge) atoms are turned into atoms with positive or negative charges.
Ionzation
If the atom has more electrons than protons, then it will have a ___ charge.
negative
Protons carry a ___ charge (+1), electrons carry a ___ charge (-1), and neutrons do ___ have a charge
positive
negative
not
___ is the process of an atom or molecule acquiring a positive or negative charge by losing or gaining an electron.
Ionization
If the atom has more protons than electrons, then it will have a ___ charge.
positive
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.
negative
positive
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.
negative
negative
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.
positive
negative
neutral
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.
positive
negative
zero
The ___ ___ is an imaginary track or orbital on which electrons travel around the nucleus of an atom.
electron shell
The ___ ___ is any electron traveling on the valence shell of an atom.
valence electron
The ___ ___ is the outermost electron shell surrounding the nucleus of an atom
valence shell
Electrons travel around the nucleus of the atom at incredibly fast speeds along imaginary tracks called orbitals called ___ ___.
electron shells
Each of the orbitals in an atom can hold a ___ number of electrons.
specific
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 ___.
filled
stable
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.
2
8
18
32
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?
12 electrons
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.
2
8
2
The electrons in the valence shell are called ___ ___.
valence electrons
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 ___.
more
full
What dictates the bonding behavior of the atom?
electrons
___ are a group of atoms that are bonded together; they are the smallest unit of matter that can participate in chemical reactions.
Molecules
___ are formed when one or more atoms bind together.
Compounds
___ ___ is atomic bonding that occurs when atoms share valence electrons
Covalent bonding
___ ___ is atomic bonding due to electrostatic attraction between two oppositely charged ions
Ionic bonding
___ ___ 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
Hydrogen bonding
A positively charged ion is called a ___.
cation
A negatively charged ion is called an ___.
anion
What is the degree of how capable an atom is of attracting the electrons of another atom?
electronegativity
A ___ bond (___ covalent bond) occurs when atoms that engage in bonding have a small difference in electrical charges.
polar
polar
A ___ bond (pure ___ covalent bond) occurs when there is no electronegativity.
nonpolar
nonpolar
A ___ is a pair of oppositely charged ions that form a bond
Dipole
When atoms bind together, they form a ___.
compound
Compounds form larger particles called ___.
molecules
A molecule is a ___ of atoms that are bonded together.
group
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).
properties
Chemical bonding occurs when ___ are shared with, given to, or taken away from another atom.
electrons
Ionic bonding happens specifically between two ___ charged ions.
oppositely
What are the three main types of bonding?
ionic bonding
covalent bonding
hydrogen bonding
There are three main types of chemical bonding: ___ bonding, ___ bonding, and ___ bonding.
ionic
covalent
hydrogen
Remember that ions are charged atoms with ___ or ___ electrons than protons (never equal).
more
fewer
What type of bonding occurs when an atom gains or loses electrons and becomes either positively or negatively charged as a result?
ionic bonding
In ionic bonding, atoms gain or lose ___ and become positively or negatively charged as a result.
electrons
An ionic bond exists when two oppositely ___ ions are bonded due to the electrostatic attraction between the two.
charged
Ionic bonds are most common between which two materials?
metal and nonmetals
___ ___ occurs when atoms share valence electrons between them to complete both of their outer shells.
Covalent bonding
What do atoms share when they have a covalent bond to complete both of their outer shells?
valence electrons
Nonmetals tend to engage in ___ bonds with each other, while bonds between metals and nonmetals are typically ___ in nature.
covalent
ionic
Which kind of elements engage in covalent bonds with each other? Which kind of elements engage in ionic bonds with each other?
nonmetals
metals with nonmetals
When valence electrons are shared equally between atoms, they are said to have a ___ bond.
nonpolar
What are the two primary types of covalent bonds?
polar covalent bonds
nonpolar covalent bonds
If electrons are shared equally, there is ___ difference in the electronegativity of the atoms involved in bonding. This occurs in ___ bonds.
no
nonpolar
In covalent bonding, the electrons are shared in order for all the atoms involved in the bond to have ___ shells.
full
Why do atoms engage in covalent bonding?
the electrons are shared in order for all the atoms involved in the bond to have full shells
Electrons that are shared unequally have a stronger electrical pull on the electrons. This occurs in ___ bonds.
polar
When electrons are shared unequally, they are said to have a ___ bond.
polar
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).
small
larger
___ ___ occurs when an atom within molecule bonds with a hydrogen atom.
Hydrogen bonding
H2O is a ___ covalent molecule – the electrons are slightly closer to the oxygen atom.
polar
One of the most common places we see hydrogen bonding is between ___ molecules.
water
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.
negative
positive
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.
not
hydrogen
A ___ ___ is a chemical combination of two or more elements.
chemical compound
How many bonds do alkanes have between their carbon atoms?
one (single bonds)
___ are organic compounds that have only a single bond between their carbon atoms.
Alkanes
___ are organic compounds that have at least one double bond between their carbon atoms.
Alkenes
___ are organic compounds that have at least one triple bond between their carbon atoms.
Alkynes
How many bonds do alkynes have between their carbon atoms?
3 (triple bonds)
There are several compounds that are only composed of hydrogen and carbon. The compounds that only consist of hydrogen and carbon are called ___ ___.
organic compounds
Alkanes have only a ___ bond between their carbon atoms.
single
What are the three types of hydrocarbons?
alkanes
alkenes
alkynes
How many bonds do alkenes have between their carbon atoms?
2 (double bonds)
A ___ is made up of chemically bonded atoms of individual elements.
compound
Methane (CH4), Ethane (C2H6), Propane (C3H8), and Butane (C4H10) are examples of ___.
alkanes
As you may have noticed, the suffix of the alkanes all end in “___”.
“ane”
Alkenes have at least one ___ bond between one set of carbon atoms.
double
Ethene (C2H4), Propene, 1-Butene, 2-pentene are examples of ____.
alkenes
Alkynes have at least one ___ bond between two of their carbon atoms.
triple
As you may have noticed, the suffix of the alkenes all end in “___”.
“-ene”
Ethyne, 1-propyne, 1-butyne, 1-pentyne arre examples of ___.
alkynes
Note, the suffix of the alkynes all end in “___”.
“-yne”
Hydrocarbons with a single bond are known as ___.
alkanes
Hydrocarbons with a triple bond are known as ___.
alkynes
Hydrocarbons with a double bond are known as ___.
alkenes
Hydrocarbons are organic compounds made up of only ___ (H) and ___ (C).
hydrogens
carbons
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?
hydrocarbon prefixes
___ are hydrocarbons that contain only single bonds.
Alkanes
___ are hydrocarbons that contain at least one double bond.
Alkenes
___ are hydrocarbons that contain at least one triple bond.
Alkynes
The name of a hydrocarbon depends on the number of ___ that it has in its main chain.
carbons
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 ___.
longest
carbons
How many carbons does the prefix Meth- signify?
1
How many carbons does the prefix Eth- signify?
2
How many carbons does the prefix Prop- signify?
3
How many carbons does the prefix But- signify?
4
How many carbons does the prefix Penta- signify?
5
How many carbons does the prefix Hexa- signify?
6
How many carbons does the prefix Hepta- signify?
7
How many carbons does the prefix Octa- signify?
8
How many carbons does the prefix Nona- signify?
9
How many carbons does the prefix Deca- signify?
10
Then, the ___ that will be given to the hydrocarbon depends on whether it is an alkane, an alkene, or an alkyne,
suffix
What suffix do hydrocarbons have that are alkanes?
-ane
What suffix do hydrocarbons have that are alkenes?
-ene
What suffix do hydrocarbons have that are alkynes?
-yne
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 ___.
longest
carbon
hepta-
-yne
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
position
double
Which organic compounds contain the hydroxyl group (-OH) bonded to a saturated carbon atom?
Alcohols
What is the general formula for alcohols?
R-OH
___ have the general formula R-OH, where R is an alkyl group.
Alcohols
Alcohols are named by adding the suffix “___” after the prefix of the main alkyl chain.
“-ol”
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 ___.
2
1-propanol
(“prop-” + “-ane-” + “-ol”)
To recognize an alcohol, just look for the “___” group!
“-OH”
What is the structure of methanol?
CH3OH
*The structure of methanol is an alcohol in which R is a methyl group ( −CH3 )
___ are organic compounds that contain two alkyl groups linked by an oxygen atom.
Ethers
An ___ ___ is a radical that is formed by removing a hydrogen atom from an alkane chain.
alkyl group
___ have the general formula ROR’.
Ethers
Ethers have the general formula ___, where R and R’ are alkyl groups
ROR’
How many ways are there to name ethers?
2
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.
longer
shorter
ethane
alkoxy
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 ___ ___).
separately
ethyl
propyl
dimethyl ether
To recognize an ether, just look for the ___ group!
C-O-C
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 ___.
ester
An ___ is an organic compound that contains a carbonyl group bonded to an alkyl group and a hydrogen atom.
Aldehyde
An ___ group is a radical that is formed by removing a hydrogen atom from an alkane chain.
alkyl
A ___ group is a functional group that contains a carbon atom forming a double bond with an oxygen atom (C=O).
carbonyl
___ have the general formula RCHO (it is not written RCOH to avoid confusing an aldehyde with an alcohol).
Aldehydes
Aldehydes have the general formula ___.
RCHO
Aldehydes are named by using the prefix of the parent alkane chain and adding the suffix “___”.
For example, the aldehyde CH3CHO would be named “___”.
“-al”
ethanal
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.
“-aldehyde”
An ___ is an organic compound that contains a carbonyl group (C=O) bonded to an alkyl group (-R) and a hydrogen atom (-H).
aldehyde
A ___ group is a functional group that contains a carbon atom forming a double bond with an oxygen atom (C=O).
carbonyl
___ have the general formula RCOR’ (CO is the carbonyl group, C=O).
Ketones
Ketones have the general formula ___ (CO is the carbonyl group, C=O).
RCOR’
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).
closer
2-pentanone
Ketones are named by using the prefix of the parent alkane chain and adding the suffix “___” at the end.
“-one”
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.
separately
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.
“di-“
What is the simplest and most common ketone?
acetone
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.
aldehydes
ketones
___ ___ are organic compounds that contain a carbonyl group (C=O) bonded to an alkyl group (-R) and a hydroxyl group (-OH).
Carboxylic acid
Carboxylic acids have the general formula ___ (CO is the carbonyl group, C=O).
RCOOH
___ ___ have the general formula RCOOH (CO is the carbonyl group, C=O).
Carboxylic acids
The ___ group is also known as the carboxylate group.
-COOH
Carboxylic acids are named by using the prefix of the parent alkane chain and adding the suffix “___ ___” at the end
“-anoic acid”
For example, the carboxylic acid CH3CH2CH2COOH would be named ___ ___.
butanoic acid
What are the two classes of carboxylic acids with great biological importance?
fatty acids
amino acids
___ ___ 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.
Fatty acids
unsaturated
saturated
An ___ is a hydrocarbon that contains at least one double bond and has the general formula CnH2n.
Alkene
A ___ is an organic aromatic cyclic compound with molecular formula C6H6.
Benzene
A ___ is an organic compound that contains 3 or more alternating double and single bonds.
Polyene
___ is a planar ring with 6 carbon atoms with equal C-C bond length. Each of the carbons is bonded to a hydrogen atom.
Benzene
Benzene is a planar ring with ___ carbon atoms with equal C-C bond length. Each of the carbons is bonded to a hydrogen atom.
6
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 ___.
unreactive
stability
___ are organic compounds that contain the amine group (−NH2).
Amines
Amines are organic compounds that contain the amine group (___).
−NH2
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
3
Amines are named using the word “___” as a substitute on the main chain.
For example, the amine CH3CH2CH2NH2 would be named ___.
“amino-“
1-aminopropane
Amines show ___ behavior, which means they’re able to donate an electron pair or accept a proton from an acid.
basic
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.
“-amine”
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.
more
Which of the following atoms has the largest atomic radius?
Mg
Be
Ra
Sr
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.
How many neutrons does an atom of Gd have?
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).
Which of the following has 35 protons, 45 neutrons, and 36 electrons?
Rh3+
Br–
P3-
Kr
Br-
How many electrons does a sodium ion (Na+) have?
10
How many valence electrons does sodium have?
1
How many valence electrons does the sulfide ion S2- have?
8
Which of the following atoms will form an ion that is larger than the neutral atom?
Na+
Al3+
Mg2+
Cl–
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).
What is the difference between rubidium-87 and rubidium-82?
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.
What is the charge on a sulfide ion?
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.
Which of the following represent isotopes of the same element?
Fe2+ and Fe3+
55Fe and 56Fe
H– and H+
Cl and Cl–
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.
What is the charge on a nitride ion?
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.
What charge will an ion of chlorine-37 have?
-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.
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.
- 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.
Which of the following subshells can hold a maximum of 6 electrons?
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
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.
It has 8 protons.
A neutral chlorine atom (Cl) has 7 electrons in its valence shell. Which of the following ions will it form?
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.
Which of the subshells given below can hold additional electrons?
6f14
4d6
3p6
2s2
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
Which of the given electron subshells needs an additional 2 electrons to have all of its orbitals completely filled?
4p3
5d6
6f12
4s1
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
The electron configurations of several atoms are listed below. Which of them is most likely to lose electrons?
1s22s22p63s23p6
1s22s22p63s2
1s22s22p4
1s22s2
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.
Which of the following represents the electron configuration of Li in LiCl?
1s2
In which of the following types of bonds are valence electrons completely donated from one atom to the other?
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.
In which of the following bonds are electrons donated from one atom to another?
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.
Which of the compounds below contains both ionic and covalent bonds?
CO2
KOH
CH4
NaCl
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.
Which of the following properties mainly determines a bond’s polarity?
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.
Which of the following bonds do you expect to be the most polar?
H-H
C-C
C-F
C-O
C-F
*The bond with the largest electronegativity difference is the most polar
Which of the following bonds do you expect to be nonpolar?
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.
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
Mg and O
Which of the following atoms would oxygen (O) form an ionic bond with?
Na
O
S
N
Na
Which of the following has the longest bond length?
C-I
C-Br
C-Cl
C-F
*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.
Which of the following will have the shortest bond length?
All bonds are the same length.
C≡N
C=N
C-N
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.
