Hydrogen is in Group 1A of the periodic table, known as the alkali metals, although it obviously isn't a metal. What is the reason for its placement in this group?
Responses
There isn't room for hydrogen on the right side of the table with other nonmetals.
There isn't room for hydrogen on the right side of the table with other nonmetals.
Hydrogen is a metal, but has an extremely low vaporization point.
Hydrogen is a metal, but has an extremely low vaporization point.
Hydrogen has the same electron configuration as alkali metals.
Hydrogen has the same electron configuration as alkali metals.
Scientists didn't want to reconfigure the periodic table after they discovered that hydrogen wasn't a metal.
There isn't room for hydrogen on the right side of the table with other nonmetals.
What element behaves MOST like magnesium (Mg)?
Responses
Sr
Sr
Si
Si
S
S
Sn
Sr
As we move from left to right across the periodic table, what is the general trend?
Responses
Metallic character decreases.
Metallic character decreases.
Electronegativity decreases.
Electronegativity decreases.
Atomic radii increase.
Atomic radii increase.
Nuclear shielding increases.
Metallic character decreases.
Consider this row in the periodic table of elements. Evaluate which element(s) is/are most likely to conduct electricity.
Responses
Carbon
Carbon
lithium and beryllium
lithium and beryllium
flourine and neon
flourine and neon
oxygen
Lithium and beryllium
Differentiate between metals and noble gases.
Responses
All electrons are different - noble gases have a full shells while metals have greater than half shells.
All electrons are different - noble gases have a full shells while metals have greater than half shells.
Metals have a nearly full shell of valence electrons while noble gases have a half shell of valence electrons.
Metals have a nearly full shell of valence electrons while noble gases have a half shell of valence electrons.
Noble gases have a full shell of valence electrons while metals have only a few valence electrons.
Noble gases have a full shell of valence electrons while metals have only a few valence electrons.
Valence electrons are different - metals have a full shell while noble gases have less than half a shell.
Noble gases have a full shell of valence electrons while metals have only a few valence electrons.
The main-group elements are the forty-four elements that occupy groups 1A-VIIIA of the periodic table. Main-group elements are important because of their high natural abundance both in the Earth's crust and in the human body and are commercially valuable. Review the families containing main group elements and locate families IVA - VIIA. When forming chemical compounds, these four families have commonalities. Explain using as many answer choices that would apply.
Responses
As nonmetals, they have high electron affinities.
As nonmetals, they have high electron affinities.
They gain or share electrons when they react with other elements.
They gain or share electrons when they react with other elements.
When forming compounds they become positive ions.
When forming compounds they become positive ions.
When forming compounds, they obey the octet rule to have eight outer electrons.
When forming compounds, they obey the octet rule to have eight outer electrons.
These elements form covalent bonds when combining with metals.
They gain or share electrons when they react with other elements.
When forming compounds, they obey the octet rule to have eight outer electrons.
Sodium chloride, better known as table salt, is an ionic compound. Which conclusion would best be drawn from this information?
Responses
Sodium chloride is very flexible at room temperature.
Sodium chloride is very flexible at room temperature.
Sodium chloride will not dissolve in water.
Sodium chloride will not dissolve in water.
Sodium chloride has a high melting point.
Sodium chloride has a high melting point.
Sodium chloride is a liquid at room temperature.
Sodium chloride has a high melting point.
You are studying the differences between ionic and covalent compounds. After studying the properties of each type of compound, your teacher has provided this table and asked you to (1) identify the ionic compound(s) and explain your choice(s).
Responses
Compounds A and D because they have relatively high melting points.
Compounds A and D because they have relatively high melting points.
Compound B because it has a very high melting point.
Compound B because it has a very high melting point.
Compounds A, B, and C because they are solid at room temperature.
Compounds A, B, and C because they are solid at room temperature.
Compounds A, B and C because they are soluble in water.
Compounds A, B and C because they are soluble in water.
Compounds A and D because the conduct electricity in aqueous solutions.
Compounds A and D because they have relatively high melting points.
Which statement about covalent bonds is true?
Responses
Covalent bonds are generally stronger than ionic bonds because they form full oppositely charged particles.
Covalent bonds are generally stronger than ionic bonds because they form full oppositely charged particles.
Covalent bonds are generally weaker than ionic bonds because they form full oppositely charged particles.
Covalent bonds are generally weaker than ionic bonds because they form full oppositely charged particles.
Covalent bonds are generally weaker than ionic bonds because they overlap electrons to fill their outer shell.
Covalent bonds are generally weaker than ionic bonds because they overlap electrons to fill their outer shell.
Covalent bonds are generally stronger than ionic bonds because they overlap electrons to fill their outer shell.
Covalent bonds are generally weaker than ionic bonds because they overlap electrons to fill their outer shell.
The formation of lithium fluoride (seen here) is due to
Responses
the addition of an outer (higher) energy level in the fluoride ion.
the addition of an outer (higher) energy level in the fluoride ion.
increased stability in the completion of fluorine's outer shell.
increased stability in the completion of fluorine's outer shell.
decreased attraction between the lithium and fluoride ions.
decreased attraction between the lithium and fluoride ions.
a stronger pull by the lithium atom on its valence electron.
Increased stability in the completion of fluorine's outer shell.
Identify which bond type (ionic or covalent) is present in each of the following compounds:
NaCL
CO2
CaO
Al2O3
CH4
NH3
NaCl - Ionic bond
CO2 - Covalent bond
CaO - Ionic bond
Al2O3 - Ionic bond
CH4 - Covalent bond
NH3 - Covalent bond
Which elements will bond ionically with barium such that the formula would be written as BaX2
Responses
Oxygen and Sulfur
Oxygen and Sulfur
Chlorine, Iodine, and Fluorine
Chlorine, Iodine, and Fluorine
Hydrogen, Bromine and Aluminum
Hydrogen, Bromine and Aluminum
Nitrogen, Chlorine, and Sodium
Oxygen and Sulfur
Which combination of elements below will bond ionically and in the same ratio as lithium when it bonds to sulfur?
Responses
sodium and oxygen
sodium and oxygen
carbon and oxygen
carbon and oxygen
calcium and nitrogen
calcium and nitrogen
aluminum and chlorine
Sodium and oxygen
What is the chemical formula for aluminum fluoride?
Responses
AlF
AlF
AlF3
AlF, 3
Al3F
Al, 3, F
AlFl3
AlF3
The chemical formula for sodium fluoride is
Responses
NaF2
NaF, 2
Na7F
Na, 7, F
NaF7
NaF, 7
NaF
NaF
Elements that do not have full outer electron shells will donate, share, or take electrons from other atoms. Choose the items that have the correct binary ionic formula. (Choose 2)
Responses
Potassium and sulfur form KS2
Potassium and sulfur form KS, 2
Sodium and calcium form Na2Ca
Sodium and calcium form Na, 2, Ca
Lithium and fluorine form LiF
Lithium and fluorine form LiF
Magnesium and chlorine form MgCl2
Magnesium and chlorine form MgCl, 2
Strontium and oxygen form Sr2O2
Strontium and oxygen form Sr, 2, O, 2
Lithium and fluorine form LiF
Magnesium and chlorine form MgCl2
NH3 is nitrogen trihydride (ammonia) and BF3 is boron trifluoride. What is the name for AlCl3 and why?
Responses
Aluminum trichloride - It has the prefix "tri-" since it has the same ratio as the other compounds.
Aluminum trichloride - It has the prefix "tri-" since it has the same ratio as the other compounds.
Aluminum chloride - It does not have the prefix "tri-" since it is ionic.
Aluminum chloride - It does not have the prefix "tri-" since it is ionic.
Aluminum chloride - Ionic compounds do not get a prefix on the first name if there is only one of that element.
Aluminum chloride - Ionic compounds do not get a prefix on the first name if there is only one of that element.
Monoaluminum trichloride - There is only one aluminum and it needs the prefix "mono-".
Aluminum chloride - Ionic compounds do not get a prefix on the first name if there is only one of that element.
Which formulas and their respective names DO NOT match?
I) BaO barium hydroxide
II) CCl4 carbon tetrachloride
III) N2O4 dinitrogen tetroxide
IV) HF monohydrogen monofluoride
Responses
I and II
I and II
II and III
II and III
I and IV
I and IV
I, III and IV
I and II
Using IUPAC nomenclature, give the name of BH3 and AlH3 and elaborate why that name is correct.
Responses
boron trihydride & aluminum trihydride - both molecules combine two non-metals and form covalent bonds.
boron trihydride & aluminum trihydride - both molecules combine two non-metals and form covalent bonds.
boron hydride & aluminum hydride - both compounds combine a main group metal and a non-metal to form ionic bonds.
boron hydride & aluminum hydride - both compounds combine a main group metal and a non-metal to form ionic bonds.
boron hydride - boron is a main group metal and hydrogen is a non-metal and they form ionic bonds.
aluminum trihydride - aluminum and hydrogen are both non-metals and form covalent bonds.
boron hydride - boron is a main group metal and hydrogen is a non-metal and they form ionic bonds., , aluminum trihydride - aluminum and hydrogen are both non-metals and form covalent bonds.
boron trihydride - boron and hydrogen are both non-metals and form covalent bonds.
aluminum hydride - aluminum is a main group metal and hydrogen is a non-metal and they form ionic bonds.
boron trihydride - boron and hydrogen are both non-metals and form covalent bonds.
aluminum hydride - aluminum is a main group metal and hydrogen is a non-metal and they form ionic bonds.
The name "boron trihydride" is correct because boron is a non-metal and hydrogen is also a non-metal, so they form covalent bonds.
The name "aluminum hydride" is correct because aluminum is a main group metal and hydrogen is a non-metal, so they form ionic bonds.
Determine the correct name for the compound, Mg3N2.
Responses
Magnesium nitride
Magnesium nitride
Trimagnesium dinitride
Trimagnesium dinitride
Magnesium (II) nitride
Magnesium (II) nitride
Manganese nitride
Magnesium nitride
The main-group elements are the forty-four elements that occupy groups 1A-VIIIA of the periodic table. Main-group elements are important because of their high natural abundance both in the Earth's crust and in the human body and are commercially valuable. Review the families containing main group elements and locate families IVA - VIIA. When forming chemical compounds, these four families have commonalities. Explain using as many answer choices that would apply.
Responses
As nonmetals, they have high electron affinities.
As nonmetals, they have high electron affinities.
They gain or share electrons when they react with other elements.
They gain or share electrons when they react with other elements.
When forming compounds they become positive ions.
When forming compounds they become positive ions.
When forming compounds, they obey the octet rule to have eight outer electrons.
When forming compounds, they obey the octet rule to have eight outer electrons.
These elements form covalent bonds when combining with metals.
They gain or share electrons when they react with other elements.
When forming compounds, they obey the octet rule to have eight outer electrons.
.
The main-group elements in families IVA to VIIA gain or share electrons when they react with other elements. They also obey the octet rule when forming compounds, meaning they strive to have eight electrons in their outermost electron shell. These elements can form both ionic and covalent bonds, depending on the specific elements involved in the compound.
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I apologize for the previous confusion. Let me clarify and provide a more concise answer:
The main-group elements in families IVA to VIIA have commonalities when forming chemical compounds. They tend to gain or share electrons when they react with other elements. In forming compounds, they obey the octet rule, meaning they strive to have eight electrons in their outermost electron shell. Additionally, these elements can form both ionic and covalent bonds with other elements depending on the specific elements involved in the compound.