If only an element’s atomic number and weight are provided, what other atomic information can be determined for a neutral atom?(1 point)
Responses
only the valence electrons
only the valence electrons
only the number of protons and electrons
only the number of protons and electrons
the number of protons, electrons and neutrons
the number of protons, electrons and neutrons
only the number of protons and neutrons
29 answers
the number of protons, electrons and neutrons
What quality differentiates hydrogen (H) from the other elements in group 1, the alkali metals?(1 point)
Responses
It is found by itself in nature.
It is found by itself in nature.
It has more than one valence electron.
It has more than one valence electron.
It is not very reactive.
It is not very reactive.
It is a non-metal.
Responses
It is found by itself in nature.
It is found by itself in nature.
It has more than one valence electron.
It has more than one valence electron.
It is not very reactive.
It is not very reactive.
It is a non-metal.
It is found by itself in nature.
On which atomic property proposed by Henry Moseley is the current periodic table of the elements based?(1 point)
Responses
electric charge
electric charge
nucleus size
nucleus size
atomic weight
atomic weight
atomic number
Responses
electric charge
electric charge
nucleus size
nucleus size
atomic weight
atomic weight
atomic number
atomic number
Which incorrect aspect of Rutherford’s model was fixed by Bohr’s model?(1 point)
Responses
Atoms have small, dense, positively charged nuclei.
Atoms have small, dense, positively charged nuclei.
Electrons move freely in curved paths around the nucleus.
Electrons move freely in curved paths around the nucleus.
The nucleus contains most of the mass of an atom.
The nucleus contains most of the mass of an atom.
Positively charged nuclei repel positively charged alpha particles.
Responses
Atoms have small, dense, positively charged nuclei.
Atoms have small, dense, positively charged nuclei.
Electrons move freely in curved paths around the nucleus.
Electrons move freely in curved paths around the nucleus.
The nucleus contains most of the mass of an atom.
The nucleus contains most of the mass of an atom.
Positively charged nuclei repel positively charged alpha particles.
Electrons move freely in curved paths around the nucleus.
You plan to pass alpha particles through a field that contains a consistent type of particle. Which configuration will result in the largest deflection of alpha particles? (1 point)
Responses
high-energy alpha particles passing through a field of low mass-number-particles
high-energy alpha particles passing through a field of low mass-number-particles
high-energy alpha particles passing through a field of high mass-number-particles
high-energy alpha particles passing through a field of high mass-number-particles
low-energy alpha particles passing through a field of low mass-number-particles
low-energy alpha particles passing through a field of low mass-number-particles
low-energy alpha particles passing through a field of high mass-number-particles
Responses
high-energy alpha particles passing through a field of low mass-number-particles
high-energy alpha particles passing through a field of low mass-number-particles
high-energy alpha particles passing through a field of high mass-number-particles
high-energy alpha particles passing through a field of high mass-number-particles
low-energy alpha particles passing through a field of low mass-number-particles
low-energy alpha particles passing through a field of low mass-number-particles
low-energy alpha particles passing through a field of high mass-number-particles
high-energy alpha particles passing through a field of low mass-number-particles
Which statement about metals and nonmetals is correct?(1 point)
Responses
Most metals are a solid under normal conditions, and most nonmetals are a liquid.
Most metals are a solid under normal conditions, and most nonmetals are a liquid.
Metals tend to be poor conductors of electricity, while nonmetals are strong conductors of electricity.
Metals tend to be poor conductors of electricity, while nonmetals are strong conductors of electricity.
Metals can be hammered into thin sheets, and nonmetals are brittle.
Metals can be hammered into thin sheets, and nonmetals are brittle.
Metals and nonmetals can both be found in any column of the periodic table.
Responses
Most metals are a solid under normal conditions, and most nonmetals are a liquid.
Most metals are a solid under normal conditions, and most nonmetals are a liquid.
Metals tend to be poor conductors of electricity, while nonmetals are strong conductors of electricity.
Metals tend to be poor conductors of electricity, while nonmetals are strong conductors of electricity.
Metals can be hammered into thin sheets, and nonmetals are brittle.
Metals can be hammered into thin sheets, and nonmetals are brittle.
Metals and nonmetals can both be found in any column of the periodic table.
Metals can be hammered into thin sheets, and nonmetals are brittle.
Which statement best explains why hydrogen’s atomic number is equal to its mass?(1 point)
Responses
Hydrogen is stable, with two electrons in its outer shell.
Hydrogen is stable, with two electrons in its outer shell.
Hydrogen only has one electron
Hydrogen only has one electron
Hydrogen is in the first row and the first column of the periodic table.
Hydrogen is in the first row and the first column of the periodic table.
Hydrogen does not have any neutrons.
Responses
Hydrogen is stable, with two electrons in its outer shell.
Hydrogen is stable, with two electrons in its outer shell.
Hydrogen only has one electron
Hydrogen only has one electron
Hydrogen is in the first row and the first column of the periodic table.
Hydrogen is in the first row and the first column of the periodic table.
Hydrogen does not have any neutrons.
Hydrogen only has one electron
Question
Use the periodic table to answer the question.
An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4
Which statement correctly compares the valence electrons for atoms of francium (Fr) and barium (Ba)?
(1 point)
Responses
Barium has fewer valence electrons, but they are in a higher energy level.
Barium has fewer valence electrons, but they are in a higher energy level.
Francium has fewer valence electrons, but they are in a higher energy level.
Francium has fewer valence electrons, but they are in a higher energy level.
Francium has more valence electrons, and they are in a higher energy level.
Francium has more valence electrons, and they are in a higher energy level.
Barium has more valence electrons, and they are in a higher energy level.
Barium has more valence electrons, and they are in a higher energy level.
Skip to navigation
Use the periodic table to answer the question.
An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4
Which statement correctly compares the valence electrons for atoms of francium (Fr) and barium (Ba)?
(1 point)
Responses
Barium has fewer valence electrons, but they are in a higher energy level.
Barium has fewer valence electrons, but they are in a higher energy level.
Francium has fewer valence electrons, but they are in a higher energy level.
Francium has fewer valence electrons, but they are in a higher energy level.
Francium has more valence electrons, and they are in a higher energy level.
Francium has more valence electrons, and they are in a higher energy level.
Barium has more valence electrons, and they are in a higher energy level.
Barium has more valence electrons, and they are in a higher energy level.
Skip to navigation
Barium has fewer valence electrons, but they are in a higher energy level.
Why are the noble gases the least reactive elements? (1 point)
Responses
They are the most electronegative elements.
They are the most electronegative elements.
They have a full valence electron shell.
They have a full valence electron shell.
They have an empty inner electron shell.
They have an empty inner electron shell.
They are the elements with the smallest atomic mass.
Responses
They are the most electronegative elements.
They are the most electronegative elements.
They have a full valence electron shell.
They have a full valence electron shell.
They have an empty inner electron shell.
They have an empty inner electron shell.
They are the elements with the smallest atomic mass.
They have a full valence electron shell.
Group 2 elements have two valence electrons. Which kind of bond will they most likely form, and why?(1 point)
Responses
A covalent bond is likely because they want to share those two valence electrons in order to become stable.
A covalent bond is likely because they want to share those two valence electrons in order to become stable.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
A metallic bond is likely because they are metals and can bond with other metals.
A metallic bond is likely because they are metals and can bond with other metals.
An ionic bond is likely because they are metals and will want to bond with nonmetals.
Responses
A covalent bond is likely because they want to share those two valence electrons in order to become stable.
A covalent bond is likely because they want to share those two valence electrons in order to become stable.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
A metallic bond is likely because they are metals and can bond with other metals.
A metallic bond is likely because they are metals and can bond with other metals.
An ionic bond is likely because they are metals and will want to bond with nonmetals.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
What type of bonds are present in the compound carbon tetrachloride (CCl4)? (1 point)
Responses
Hydrogen bonds because there are hidden hydrogens in the compound.
Hydrogen bonds because there are hidden hydrogens in the compound.
Metallic bonds because carbon is a positively charged atom.
Metallic bonds because carbon is a positively charged atom.
Covalent bonds because both carbon and chlorine are nonmetals.
Covalent bonds because both carbon and chlorine are nonmetals.
Ionic bonds because chlorine donates electrons to carbon.
Responses
Hydrogen bonds because there are hidden hydrogens in the compound.
Hydrogen bonds because there are hidden hydrogens in the compound.
Metallic bonds because carbon is a positively charged atom.
Metallic bonds because carbon is a positively charged atom.
Covalent bonds because both carbon and chlorine are nonmetals.
Covalent bonds because both carbon and chlorine are nonmetals.
Ionic bonds because chlorine donates electrons to carbon.
Covalent bonds because both carbon and chlorine are nonmetals.
An element has six valence electrons. Which ionic charge will its ion carry?(1 point)
Responses
6–
6–
2+
2+
2–
2–
6+
Responses
6–
6–
2+
2+
2–
2–
6+
2-
How many electrons can carbon accept from other atoms while bonding? (1 point)
Responses
six
six
two
two
eight
eight
four
Responses
six
six
two
two
eight
eight
four
four
Which key difference between carbon and silicon makes carbon better suited to forming molecules for living things?(1 point)
Responses
Carbon has a greater atomic mass, allowing for stronger molecules.
Carbon has a greater atomic mass, allowing for stronger molecules.
Oxidized carbon is a gas at room temperature, rather than a solid.
Oxidized carbon is a gas at room temperature, rather than a solid.
Carbon has the right number of outer electrons to form a wide range of molecules.
Carbon has the right number of outer electrons to form a wide range of molecules.
Carbon is a naturally occurring element, so it is readily available.
Responses
Carbon has a greater atomic mass, allowing for stronger molecules.
Carbon has a greater atomic mass, allowing for stronger molecules.
Oxidized carbon is a gas at room temperature, rather than a solid.
Oxidized carbon is a gas at room temperature, rather than a solid.
Carbon has the right number of outer electrons to form a wide range of molecules.
Carbon has the right number of outer electrons to form a wide range of molecules.
Carbon is a naturally occurring element, so it is readily available.
Carbon has the right number of outer electrons to form a wide range of molecules.
Which structure defines the hydroxyl functional group?(1 point)
Responses
CH3
CH 3
OH
OH
NH2
NH 2
SH
Responses
CH3
CH 3
OH
OH
NH2
NH 2
SH
OH
1 answer