Based on properties of elements in the periodic table, which element is the best conductor of thermal energy? (1 point) Responses germanium (Ge) germanium (Ge) argon (Ar) argon (Ar) polonium (Po) polonium (Po) vanadium (V)
Polonium (Po)
Which statement best explains why hydrogen’s atomic number is equal to its mass?(1 point) Responses Hydrogen does not have any neutrons. Hydrogen does not have any neutrons. Hydrogen is stable, with two electrons in its outer shell. Hydrogen is stable, with two electrons in its outer shell. 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 only has one electron
Hydrogen only has one electron.
Which statement correctly compares the valence electrons for atoms of francium (Fr) and barium (Ba)? (1 point) Responses 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. 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. 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. Barium has fewer valence electrons, but they are in a higher energy level.
Francium has one valence electron, while barium has two valence electrons. Therefore, barium has more valence electrons, but they are in a higher energy level. The correct statement is: Barium has more valence electrons, but they are in a higher energy level.
Gallium has an atomic number of 31 and a mass number of 70. Which table shows the number of protons, neutrons, and electrons in a gallium ion with a +3 charge?(1 poin
To determine the number of protons, neutrons, and electrons in a gallium ion with a +3 charge, we need to subtract the charge from the atomic number and mass number.
The atomic number of gallium is 31, so it has 31 protons.
The mass number of gallium is 70, so it has 70 neutrons.
To determine the number of electrons, we need to consider the charge. A +3 charge means that the ion has lost 3 electrons. Since neutral gallium has 31 electrons, a +3 ion would have 31 - 3 = 28 electrons.
Therefore, the table would show:
Protons: 31
Neutrons: 70
Electrons: 28
The Periodic Table Unit Test 7 of 187 of 18 Items Question Which is true about stable isotopes?(1 point) Responses Isotopes with more neutrons than protons are always stable. Isotopes with more neutrons than protons are always stable. A stable nucleus has a similar number of protons and neutrons. A stable nucleus has a similar number of protons and neutrons. Isotopes that are naturally occurring in nature are always unstable. Isotopes that are naturally occurring in nature are always unstable. Isotopes are always unstable because they are radioactive.
A stable nucleus has a similar number of protons and neutrons.
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
The current periodic table of the elements is based on the atomic number, which was proposed by Henry Moseley.
The Periodic Table Unit Test 9 of 189 of 18 Items Question Which incorrect aspect of Rutherford’s model was fixed by Bohr’s model?(1 point) Responses Electrons move freely in curved paths around the nucleus. Electrons move freely in curved paths around the nucleus. Atoms have small, dense, positively charged nuclei. Atoms have small, dense, positively charged nuclei. 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.
The Periodic Table Unit Test 10 of 1810 of 18 Items Question 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 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 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 high 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
The configuration that will result in the largest deflection of alpha particles is when high-energy alpha particles pass through a field of low mass-number particles. So, the correct response is: high-energy alpha particles passing through a field of low mass-number particles.
11 of 1811 of 18 Items Question Where on the periodic table do you find elements that have full valence electron shells?(1 point) Responses on the left side of the periodic table on the left side of the periodic table across the top of the periodic table across the top of the periodic table on the right side of the periodic table on the right side of the periodic table across the bottom of the periodic table across the bottom of the periodic table
Elements that have full valence electron shells are found on the right side of the periodic table. So, the correct response is: on the right side of the periodic table.
Which element would have a full outer shell of electrons if it gained three electrons? (1 point) Responses argon argon lithium lithium nitrogen nitrogen boron boron
Argon (Ar)
Which group of elements has the most similar chemical properties? (1 point) Responses uranium, plutonium, and lead uranium, plutonium, and lead aluminum, silicon, and phosphorus aluminum, silicon, and phosphorus carbon, nitrogen, and oxygen carbon, nitrogen, and oxygen fluorine, chlorine, and iodine
Fluorine, chlorine, and iodine
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 an empty inner electron shell. They have an empty inner electron shell. They have a full valence electron shell. They have a full valence electron shell. They are the elements with the smallest atomic mass.
The noble gases are the least reactive elements because 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 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 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 are metals and will want to bond with nonmetals. An ionic bond is likely because they are metals and will want to bond with nonmetals. 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. Skip to navigation
Group 2 elements have two valence electrons and they are metals. Therefore, an ionic bond is likely because they will want to give away their two valence electrons in order to become stable. The correct response is: An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
An element has six valence electrons. Which ionic charge will its ion carry?(1 point) Responses 6+ 6+ 2– 2– 2+ 2+ 6– 6–
An element with six valence electrons typically forms ions with a charge of 2- in order to achieve a stable electron configuration. Hence, the correct response is: 2-.
Moving from the element with atomic number 10 to atomic number 11 on the periodic table, there is a change in reactivity. In three to five sentences, identify the direction of the change, and give two reasons for the change.
Moving from the element with atomic number 10, which is neon (Ne), to atomic number 11, which is sodium (Na), there is a change in reactivity. The reactivity generally increases. Two reasons for this change are:
1. The increase in the number of valence electrons: Neon has a full valence shell with eight electrons, making it stable and less likely to form chemical bonds. On the other hand, sodium has one valence electron that it wants to lose to achieve a stable electron configuration. This makes sodium more reactive.
2. The decrease in effective nuclear charge: As you move from neon to sodium, the atomic number increases, but so does the number of electron shells. This leads to a larger atomic radius and a decrease in the attraction between the nucleus and valence electrons. Consequently, it becomes easier for sodium to lose its valence electron, making it more reactive.
In summary, the change in reactivity from neon to sodium is an increase, primarily due to the presence of only one valence electron in sodium and a larger atomic radius resulting in decreased effective nuclear charge.
The periodic table is arranged by various patterns. Is there a pattern with regard to ionic charge? In three to five sentences, explain your reasoning and provide specific examples.
Yes, there is a pattern with regard to ionic charge in the periodic table. It can be observed by looking at the groups or columns in the table. Elements in the same group have similar chemical properties, including similar ionic charges.
For example, Group 1 elements (alkali metals) in the first column of the periodic table, such as lithium (Li), sodium (Na), and potassium (K), all have a 1+ ionic charge. They easily lose one electron to achieve a stable electron configuration.
Further, Group 2 elements (alkaline earth metals) in the second column, such as beryllium (Be), magnesium (Mg), and calcium (Ca), all have a 2+ ionic charge. They lose two electrons to obtain a stable electron configuration.
Similarly, Group 17 elements (halogens) in the seventeenth column, including fluorine (F), chlorine (Cl), and iodine (I), all have a 1- ionic charge. They easily gain one electron to achieve a stable electron configuration.
Therefore, a pattern can be seen in the periodic table where elements in the same group or column tend to exhibit similar ionic charges.