Introductory Topics - AP Chemistry
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The following is a modified true/false question. In it, you must decide if each individual statement is true (T) or false (F). If both are true, then you must also decide if the second statement is a correct explanation (CE) of the first statement.
I: Atoms in the alkaline earth metal group have smaller ionic radii than their atomic radii
BECAUSE
II: atoms in this group usually lose electrons in order to become ions, resulting in the ion lacking the outermost energy level present in the atom.
The following is a modified true/false question. In it, you must decide if each individual statement is true (T) or false (F). If both are true, then you must also decide if the second statement is a correct explanation (CE) of the first statement.
I: Atoms in the alkaline earth metal group have smaller ionic radii than their atomic radii
BECAUSE
II: atoms in this group usually lose electrons in order to become ions, resulting in the ion lacking the outermost energy level present in the atom.
The alkaline earth metals are the elements in group II, such as beryllium and magnesium. They want to have a complete octet in their outermost energy level, so they tend to lose two electrons to form the ionic state, which gives them the electron configuration of the noble gas in the previous energy level and thus a smaller ionic radius. Therefore, both statements are true and the second correctly explains the first.
The alkaline earth metals are the elements in group II, such as beryllium and magnesium. They want to have a complete octet in their outermost energy level, so they tend to lose two electrons to form the ionic state, which gives them the electron configuration of the noble gas in the previous energy level and thus a smaller ionic radius. Therefore, both statements are true and the second correctly explains the first.
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The elements with the smallest atomic radii tend to be found in which part of the periodic table?
The elements with the smallest atomic radii tend to be found in which part of the periodic table?
Atomic radius tends to increase down a group due to the addition of new energy levels; however, it decreases across a period due to increased shielding and increased nuclear mass. For these reasons, the elements with the smallest atomic radii would be in the upper right corner of the periodic table.
Atomic radius tends to increase down a group due to the addition of new energy levels; however, it decreases across a period due to increased shielding and increased nuclear mass. For these reasons, the elements with the smallest atomic radii would be in the upper right corner of the periodic table.
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How many of the following compounds are ionic?
How many of the following compounds are ionic?
Ionic compounds are chemical compounds made of charged ions held together by forces called ionic bonding. Ionic bonds are formed by transfers of valance electrons, which create charged atoms (ions) which are attracted to each other because they have opposite charges. This is not be confused with covalent bonding, in which atoms form an attraction by sharing electrons.
contains a positively charged 
ion and negatively charged 
ion which form an ionic bond. 
contains two positively charged 
ions and a negatively charged 
ion which form an ionic bond. 
, 
, and 
are all examples of molecules that contain covalent bonds. None of them contains any charged ions. The answer is therefore "two,"referring to the 
and 
molecules.
Ionic compounds are chemical compounds made of charged ions held together by forces called ionic bonding. Ionic bonds are formed by transfers of valance electrons, which create charged atoms (ions) which are attracted to each other because they have opposite charges. This is not be confused with covalent bonding, in which atoms form an attraction by sharing electrons.
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Which of the following is true of Valence Bond theory and Molecular Orbital theory?
Which of the following is true of Valence Bond theory and Molecular Orbital theory?
The Valence Bond theory states that covalent bonds are formed from atomic orbital overlap while the Molecular Orbital theory is the mathematical combination of atomic orbitals to produce anti bonding and bonding orbitals.
Hybridization occurs through combining atomic orbitals, a concept consistent with Valence Bond theory. Common bonds found in Valence Bond hybridization are sigma and pi bonds which overlap end-to-end or side-to-side respectively. Orbitals are combined in Molecular Orbital theory, producing either bonding or anti bonding orbitals. Molecular Orbital theory shows the destructive or constructive interference of sigma and pi bonds (displayed through bonding and anti bonding orbitals).
The Valence Bond theory states that covalent bonds are formed from atomic orbital overlap while the Molecular Orbital theory is the mathematical combination of atomic orbitals to produce anti bonding and bonding orbitals.
Hybridization occurs through combining atomic orbitals, a concept consistent with Valence Bond theory. Common bonds found in Valence Bond hybridization are sigma and pi bonds which overlap end-to-end or side-to-side respectively. Orbitals are combined in Molecular Orbital theory, producing either bonding or anti bonding orbitals. Molecular Orbital theory shows the destructive or constructive interference of sigma and pi bonds (displayed through bonding and anti bonding orbitals).
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What is the orbital hybridization for nitrogen in the molecule 
?
What is the orbital hybridization for nitrogen in the molecule
Start by drawing the Lewis structure of 
. 
has 
valence electrons.
Since the nitrogen has 
oxygen atoms bonded to it and a lone pair, the steric number must be 
. From that, we know that it must have sp2 hybridization.
Start by drawing the Lewis structure of
Since the nitrogen has
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Which of the following types of hybridization is found in the molecule shown below?
Which of the following types of hybridization is found in the molecule shown below?
Look at each of the carbon atoms in the chain. Each carbon atom has 
other atoms bonded to it. This means that the steric number of each carbon is 
. Thus, the only type of hybridization found in this molecule is sp2.
Look at each of the carbon atoms in the chain. Each carbon atom has
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What is the hybridization for the atom circled in red?
What is the hybridization for the atom circled in red?
Start by counting the number of atoms the nitrogen is bonded to. It has 
bonded atoms. The nitrogen also has a lone pair. This means the steric number of the nitrogen is 
. Thus, it must have 
hybridization.
Start by counting the number of atoms the nitrogen is bonded to. It has
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The compound hydrazine is given by the molecular formula 
. What type of intermolecular forces will govern the behavior of neighboring hydrazine molecules?
The compound hydrazine is given by the molecular formula
Hydrazine is a polar compound that possesses the requirements for hydrogen bonding: an "acidic hydrogen" (a hydrogen bonded to a highly electronegative atom such as oxygen, nitrogen or fluorine) and the presence of a lone pair. Both Nitrogen atoms in hydrazine have lone (unshared) electron pairs, and all four hydrogen atoms are "acidic," making hydrazine a candidate for intermolecular hydrogen bonding.
Hydrazine is a polar compound that possesses the requirements for hydrogen bonding: an "acidic hydrogen" (a hydrogen bonded to a highly electronegative atom such as oxygen, nitrogen or fluorine) and the presence of a lone pair. Both Nitrogen atoms in hydrazine have lone (unshared) electron pairs, and all four hydrogen atoms are "acidic," making hydrazine a candidate for intermolecular hydrogen bonding.
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The unique properties of water, namely its incredibly high heat capacity and surface tension, can be attributed to which of the following kinds of intermolecular/intramolecular forces?
The unique properties of water, namely its incredibly high heat capacity and surface tension, can be attributed to which of the following kinds of intermolecular/intramolecular forces?
The partial negative and positive charges on a water molecule allow it to be attracted to other polar water molecules, which creates the cohesive nature of water and contributes to its high surface tension and heat capacity. London dispersion and Van der Waals forces are significantly weaker than hydrogen bonding. Additionally, ionic bonding only occurs intramolecularly, so it has little effect on the intermolecular properties of water.
The partial negative and positive charges on a water molecule allow it to be attracted to other polar water molecules, which creates the cohesive nature of water and contributes to its high surface tension and heat capacity. London dispersion and Van der Waals forces are significantly weaker than hydrogen bonding. Additionally, ionic bonding only occurs intramolecularly, so it has little effect on the intermolecular properties of water.
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Which of the following atoms in the largest?
Which of the following atoms in the largest?
The atomic radii is the size of an atom when it is not bonded to any other atoms. The periodic table can be used to estimate the size of the atomic radii of atoms. As you move down the periodic table the atomic radii increase, but as you move from left to right on the periodic table, the size of the atomic radii decrease.
Sodium, aluminium, phosphorus, sulfur, and chlorine are all in the same row of the periodic table. Since the size of the atomic radii decreases as you move from left to right on the periodic table, the element furthest to the left will be the largest. Therefore, sodium is the largest atom out of the group.
The atomic radii is the size of an atom when it is not bonded to any other atoms. The periodic table can be used to estimate the size of the atomic radii of atoms. As you move down the periodic table the atomic radii increase, but as you move from left to right on the periodic table, the size of the atomic radii decrease.
Sodium, aluminium, phosphorus, sulfur, and chlorine are all in the same row of the periodic table. Since the size of the atomic radii decreases as you move from left to right on the periodic table, the element furthest to the left will be the largest. Therefore, sodium is the largest atom out of the group.
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Which of these atoms is the smallest?
Which of these atoms is the smallest?
The atomic radii is the size of an atom when it is not bonded to any other atoms. The periodic table can be used to estimate the size of the atomic radii of atoms. As you move down the periodic table the atomic radii increase, but as you move from left to right on the periodic table, the size of the atomic radii decrease.
Beryllium, magnesium, calcium, strontium, and barium are all in the same group on the periodic table, so the smallest element is the element closest to the top of the periodic table since the atoms become larger as you go down the periodic table. Therefore, the smallest atom of this group is beryllium.
The atomic radii is the size of an atom when it is not bonded to any other atoms. The periodic table can be used to estimate the size of the atomic radii of atoms. As you move down the periodic table the atomic radii increase, but as you move from left to right on the periodic table, the size of the atomic radii decrease.
Beryllium, magnesium, calcium, strontium, and barium are all in the same group on the periodic table, so the smallest element is the element closest to the top of the periodic table since the atoms become larger as you go down the periodic table. Therefore, the smallest atom of this group is beryllium.
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Which of the following is a characteristic of covalent bonds?
Which of the following is a characteristic of covalent bonds?
A covalent bond is one between two nonmetals, while an ionic bond is formed between a metal and a nonmetal. Covalent bonds also do not dissociate in aqueous solution to form cations and anions; this is a characteristic of ionic bonds. For example, 
represents a bond between a metal (
) and a nonmetal (
), and it dissociates in aqueous solution to form a cation (
) and an anion (
). In contrast, 
represents a bond between two nonmetals, and it does not dissociate in aqueous solution. Ionic compounds are also good conductors of electricity, while covalent compounds are not. This is because moving electrons are required in order to conduct electricity. When dissolved in aqueous solution, ions are free to move and thus conduct electricity. Covalent bonds have localized electrons, which cannot move and thus cannot conduct electricity well.
A covalent bond is one between two nonmetals, while an ionic bond is formed between a metal and a nonmetal. Covalent bonds also do not dissociate in aqueous solution to form cations and anions; this is a characteristic of ionic bonds. For example,
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Which of the following is an example of a nonpolar covalent bond?
Which of the following is an example of a nonpolar covalent bond?
A covalent bond is a bond between two nonmetals, in which electrons are shared. This means that 
cannot be the correct answer, as sodium is a metal. In fact, 
is a classic example of an ionic compound.
A polar covalent bond is a bond between two nonmetals in which one nonmetal is more electronegative than the other, pulling the shared electrons toward itself. This occurs in 
; chlorine is much more electronegative than hydrogen and pulls the shared electrons toward itself. This gives chlorine a partial negative charge and hydrogen a partial positive charge. 
is also an example of a polar covalent bond; oxygen is much more electronegative than hydrogen, and each oxygen in a water molecule pulls the shared electrons toward itself. This gives oxygen a partial negative charge and hydrogen a partial positive charge.
A nonpolar covalent bond is a bond between two nonmetals in which electrons are shared equally between the nonmetals. This occurs when the two nonmetals are of equal electronegativity. As the atoms of 
have the same identity (chlorine), they have the same electronegativity. Thus, electrons are shared equally between the two chlorine atoms--in a nonpolar covalent bond.
A covalent bond is a bond between two nonmetals, in which electrons are shared. This means that
A polar covalent bond is a bond between two nonmetals in which one nonmetal is more electronegative than the other, pulling the shared electrons toward itself. This occurs in
A nonpolar covalent bond is a bond between two nonmetals in which electrons are shared equally between the nonmetals. This occurs when the two nonmetals are of equal electronegativity. As the atoms of
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Which of these following diatomic molecules is joined by a double covalent bond?
Which of these following diatomic molecules is joined by a double covalent bond?
Oxygen has a valence of 6, meaning it is looking to form two covalent bonds to complete its octet. Thus, 
exists as a diatomic molecule joined by a double covalent bond. 
and 
are held together by single covalent bonds, and 
is held together by a triple covalent bond.
Oxygen has a valence of 6, meaning it is looking to form two covalent bonds to complete its octet. Thus,
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Which of the following lists bond strength in order of weakest to strongest?
Which of the following lists bond strength in order of weakest to strongest?
Dipole-dipole interactions are the weakest because they are the result of attractions between weak partial charges
Hydrogen bonds are a special type of dipole-dipole interaction, but they are much stronger.
An ionic bond is the result of the complete transfer of electrons from on atom to another. This results in a positive charge on one atom and a negative charge on the other. The charges on these ions are much stronger than in dipoles. The two oppositely charged atoms are held together by electrostatic attraction.
Atoms that are part of a covalent bond share electrons. This makes the atoms harder to separate and, therefore, the bond is very strong.
Dipole-dipole interactions are the weakest because they are the result of attractions between weak partial charges
Hydrogen bonds are a special type of dipole-dipole interaction, but they are much stronger.
An ionic bond is the result of the complete transfer of electrons from on atom to another. This results in a positive charge on one atom and a negative charge on the other. The charges on these ions are much stronger than in dipoles. The two oppositely charged atoms are held together by electrostatic attraction.
Atoms that are part of a covalent bond share electrons. This makes the atoms harder to separate and, therefore, the bond is very strong.
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Which of the following compounds contains 
covalent bonds?
Which of the following compounds contains
For this question, we're asked to determine which answer choice represents a compound with a total of six covalent bonds.
To answer this, we'll need to know the structure of each of the compounds. Moreover, it's important to remember that double bonds count as two covalent bonds.
Both sulfuric acid and phosphoric acid have a total of eight covalent bonds, while nitric acid has five. Carbonic acid is the only one shown that contains six covalent bonds, making it the correct answer.
For this question, we're asked to determine which answer choice represents a compound with a total of six covalent bonds.
To answer this, we'll need to know the structure of each of the compounds. Moreover, it's important to remember that double bonds count as two covalent bonds.
Both sulfuric acid and phosphoric acid have a total of eight covalent bonds, while nitric acid has five. Carbonic acid is the only one shown that contains six covalent bonds, making it the correct answer.
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Which of the following best explains the main difference between strong and weak acids or bases?
Which of the following best explains the main difference between strong and weak acids or bases?
Molarity has no determination in whether an acid or base is strong or weak. Rather, molarity specifies the concentration of hydroxide or hydrogen ions in a solution. Weak Acids do not completely dissociate in water, while strong acids do. Polyprotic acids, those with more than one proton to donate, do not necessarily determine if an acid is strong (e.g. hydrochloric acid is an example of a strong, monoprotic acid).
Molarity has no determination in whether an acid or base is strong or weak. Rather, molarity specifies the concentration of hydroxide or hydrogen ions in a solution. Weak Acids do not completely dissociate in water, while strong acids do. Polyprotic acids, those with more than one proton to donate, do not necessarily determine if an acid is strong (e.g. hydrochloric acid is an example of a strong, monoprotic acid).
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Is 
an atomic element, molecular element, molecular compound, or ionic compound?
Is
is an ionic compound because it is composed of a metal and a nonmetal.
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Is 
an atomic element, molecular element, molecular compound, or ionic compound?
Is
is a molecular compound because it consists of a nonmetal connected to another nonmetal.
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classifying compounds/elements
Is xenon an atomic element, molecular element, molecular compound, or ionic compound?
classifying compounds/elements
Is xenon an atomic element, molecular element, molecular compound, or ionic compound?
Xenon is an atomic element because its elemental form consists of one atom.
Xenon is an atomic element because its elemental form consists of one atom.
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