The Periodic Table - AP Chemistry
Card 1 of 950
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.
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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?
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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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The set of elements with the highest first ionization energies are known as which of the following?
The set of elements with the highest first ionization energies are known as which of the following?
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The noble gases possess a full octet of electrons. They have the largest first ionization energies because of their tendency to keep all of their valence electrons. Halogens have the highest electron affinity; therefore, they have high—but not the highest—ionization energies. The alkali and alkaline earth metals have low electron affinities and low ionization energies. Last, the metalloids possess ionization energies that are neither high nor low.
The noble gases possess a full octet of electrons. They have the largest first ionization energies because of their tendency to keep all of their valence electrons. Halogens have the highest electron affinity; therefore, they have high—but not the highest—ionization energies. The alkali and alkaline earth metals have low electron affinities and low ionization energies. Last, the metalloids possess ionization energies that are neither high nor low.
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Which of the following elements has the most metallic character: 
?
Which of the following elements has the most metallic character:
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The metallic character of elements increases as you move down a group. All of the listed elements are in Group 5. Since 
is the furthest down, it must have the most metallic character.
The metallic character of elements increases as you move down a group. All of the listed elements are in Group 5. Since
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Which of the following elements has the largest atomic radius: 
?
Which of the following elements has the largest atomic radius:
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When looking at a periodic table, you should notice that all of these elements are in the same period. Recall that atomic radii decrease as you move right on a period. Thus, this is the order of the elements by decreasing radius:
, or gallium, has the largest radius because it is the furthest left on the periodic table.
When looking at a periodic table, you should notice that all of these elements are in the same period. Recall that atomic radii decrease as you move right on a period. Thus, this is the order of the elements by decreasing radius:
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Rank the following in order of increasing metallic character: 
Rank the following in order of increasing metallic character:
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The correct answer is 
has the most nonmetallic characteristics while 
has the most metallic characteristics. According to periodic trends, metallic character decreases from left to right across a period and increases top to bottom. Therefore, 
will show less metallic character than 
.
The correct answer is
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Which of the following atoms in the largest?
Which of the following atoms in the largest?
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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?
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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 atom is the most electronegative?
Which atom is the most electronegative?
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Electronegativity refers to the ability of an atom to attract and bind electrons. If the valence electrons are less then half full, then it takes less energy to lose an electron than gain electron making these atoms less electronegative. If the valence electrons are more than half full, then it takes less energy to gain electrons compared to losing an electron; therefore these electrons are more electronegative. The periodic table can be used to predict the electronegativity of the atom and how it compares to other atoms. As you move left to right of the periodic table, the electronegativity increases because the atoms on the right side of the periodic table have more valence electrons, and smaller radii. As you move down the periodic table the electronegativity decreases because the atomic number increases resulting in a greater distance between valence electrons and the nucleus causing less pull on the valence electrons.
Using the electronegativity periodic trend, we can predict which of the atom's is most electronegative. Aluminium, silicon, phosphorous, sulfur, and chlorine are all in the same row in the periodic table. Therefore, chlorine is the most electronegative because it is the farthest right on the periodic table so it has the most valence electrons and it will cost less energy to gain an electron than lose an electron.
Electronegativity refers to the ability of an atom to attract and bind electrons. If the valence electrons are less then half full, then it takes less energy to lose an electron than gain electron making these atoms less electronegative. If the valence electrons are more than half full, then it takes less energy to gain electrons compared to losing an electron; therefore these electrons are more electronegative. The periodic table can be used to predict the electronegativity of the atom and how it compares to other atoms. As you move left to right of the periodic table, the electronegativity increases because the atoms on the right side of the periodic table have more valence electrons, and smaller radii. As you move down the periodic table the electronegativity decreases because the atomic number increases resulting in a greater distance between valence electrons and the nucleus causing less pull on the valence electrons.
Using the electronegativity periodic trend, we can predict which of the atom's is most electronegative. Aluminium, silicon, phosphorous, sulfur, and chlorine are all in the same row in the periodic table. Therefore, chlorine is the most electronegative because it is the farthest right on the periodic table so it has the most valence electrons and it will cost less energy to gain an electron than lose an electron.
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Which element is the least electronegative?
Which element is the least electronegative?
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Electronegativity refers to the ability of an atom to attract and bind electrons. If the valence electrons are less then half full, then it takes less energy to lose an electron than gain electron making these atoms less electronegative. If the valence electrons are more than half full, then it takes less energy to gain electrons compared to losing an electron; therefore these electrons are more electronegative. The periodic table can be used to predict the electronegativity of the atom and how it compares to other atoms. As you move left to right of the periodic table, the electronegativity increases because the atoms on the right side of the periodic table have more valence electrons. As you move down the periodic table the electronegativity decreases because the atomic number increases resulting in a greater distance between valence electrons and the nucleus causing less pull on the valence electrons.
Using the electronegativity periodic trend, we can predict which of the atom's is least electronegative. Oxygen, sulfur, selenium, tellurium, and polonium are all in the same group of the periodic table. Therefore, polonium is the least electronegative because it is closest to the bottom of the periodic table and has the largest atomic numbers. Since polonium has the largest atomic number, there is a greater distance between the valence electrons and the nucleus resulting in a decreased pull on the valence electrons. Therefore, it is easier to lose a valence electron compared to atom's with a smaller atomic number.
Electronegativity refers to the ability of an atom to attract and bind electrons. If the valence electrons are less then half full, then it takes less energy to lose an electron than gain electron making these atoms less electronegative. If the valence electrons are more than half full, then it takes less energy to gain electrons compared to losing an electron; therefore these electrons are more electronegative. The periodic table can be used to predict the electronegativity of the atom and how it compares to other atoms. As you move left to right of the periodic table, the electronegativity increases because the atoms on the right side of the periodic table have more valence electrons. As you move down the periodic table the electronegativity decreases because the atomic number increases resulting in a greater distance between valence electrons and the nucleus causing less pull on the valence electrons.
Using the electronegativity periodic trend, we can predict which of the atom's is least electronegative. Oxygen, sulfur, selenium, tellurium, and polonium are all in the same group of the periodic table. Therefore, polonium is the least electronegative because it is closest to the bottom of the periodic table and has the largest atomic numbers. Since polonium has the largest atomic number, there is a greater distance between the valence electrons and the nucleus resulting in a decreased pull on the valence electrons. Therefore, it is easier to lose a valence electron compared to atom's with a smaller atomic number.
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Which of the following is a transition metal?
Which of the following is a transition metal?
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Transition metals are found in the "middle" of the table
Na and Sr are metals
Cl and Po are non-metals
Transition metals are found in the "middle" of the table
Na and Sr are metals
Cl and Po are non-metals
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Which of the following elements are classified as a non-metal?
Which of the following elements are classified as a non-metal?
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Rn is radon, a noble gas, which is not a metal. As a rule, elements to the left are metals, elements to the right are non-metals. The barrier would be the elements that are immideately to the right of the transition metals
Rn is radon, a noble gas, which is not a metal. As a rule, elements to the left are metals, elements to the right are non-metals. The barrier would be the elements that are immideately to the right of the transition metals
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Li, V
As, Nb
Ir, Mn
Hg, Au
O, S
Which of the following contains a metal and a non-metal?
Li, V
As, Nb
Ir, Mn
Hg, Au
O, S
Which of the following contains a metal and a non-metal?
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Non-metals are on the right side of the periodic table—past the metaloids and metals are on the left
As and Nb are the only combination that is a metal and non-metal
Non-metals are on the right side of the periodic table—past the metaloids and metals are on the left
As and Nb are the only combination that is a metal and non-metal
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Which of the following is a metalloid?
Which of the following is a metalloid?
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Metalloids are the groups of elements that separate the metals and non-metals; these form a "stair-case" on the periodic table
Metalloids are the groups of elements that separate the metals and non-metals; these form a "stair-case" on the periodic table
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Why are the transition metals good conductors of electricity?
Why are the transition metals good conductors of electricity?
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Transition metals have only partially filled valence bands. Thus, the electrons can move among the d orbitals, and this electron flow allows the transition metals to be good conductors of electricity.
Transition metals have only partially filled valence bands. Thus, the electrons can move among the d orbitals, and this electron flow allows the transition metals to be good conductors of electricity.
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Which of the following best explains effective nuclear charge (Zeff)?
Which of the following best explains effective nuclear charge (Zeff)?
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The correct answer choice is an accurate explanation of effective nuclear charge. Since electrons are negatively charged, they are attracted to protons, which are positively charged. Protons are located in the nucleus of an atom.
The correct answer choice is an accurate explanation of effective nuclear charge. Since electrons are negatively charged, they are attracted to protons, which are positively charged. Protons are located in the nucleus of an atom.
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Which of the following is not a property of metals?
Which of the following is not a property of metals?
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The metals are found on the left side and the middle of the periodic table, and include the active metals, transition metals, and lanthanide and actinide series of elements. They easily give up electrons to form cations, since they have LOW ionization energies.
The metals are found on the left side and the middle of the periodic table, and include the active metals, transition metals, and lanthanide and actinide series of elements. They easily give up electrons to form cations, since they have LOW ionization energies.
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Which of the following does not determine the length of an element's atomic radius?
Which of the following does not determine the length of an element's atomic radius?
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The number of neutorns is the only thing out of the answer choices that does not impact an element's atomic radius. Since neutrons have no charge, they do not impact the attractive forces between electrons and protons.
The number of neutorns is the only thing out of the answer choices that does not impact an element's atomic radius. Since neutrons have no charge, they do not impact the attractive forces between electrons and protons.
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What type of element is selenium?
What type of element is selenium?
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Selenium is on the right side of the periodic table, so it is not a metal or metalloid. It is not in column 7 or 8, so it is not a halogen or noble gas. Thus, it must be a nonmetal.
Selenium is on the right side of the periodic table, so it is not a metal or metalloid. It is not in column 7 or 8, so it is not a halogen or noble gas. Thus, it must be a nonmetal.
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Which property of metals make them a good component of wiring that conducts electricity?
Which property of metals make them a good component of wiring that conducts electricity?
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Electricity is produced and conducted by the movement of electrons, and thus the most important property that allows them to be used for wiring is their valence electrons that can move freely.
Electricity is produced and conducted by the movement of electrons, and thus the most important property that allows them to be used for wiring is their valence electrons that can move freely.
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