An element with six valence electrons is typically in Group 16 of the periodic table (such as oxygen or sulfur). To achieve a stable electron configuration, it generally needs to gain two electrons. Therefore, the ionic charge of its ion will be 2–.
A) An element has six valence electrons. Which ionic charge will its ion carry? (1 point)
2+
6–
6+
2–
7 answers
molecule
describe 1-2 sentence
Points
Awarded Criteria
2 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
1 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered
describe 1-2 sentence
Points
Awarded Criteria
2 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
1 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered
A molecule is a group of two or more atoms bonded together, representing the smallest fundamental unit of a chemical compound that retains the chemical properties of that compound. Molecules can consist of the same or different types of atoms, such as the oxygen molecule (O₂) made of two oxygen atoms or water (H₂O), which is composed of two hydrogen atoms and one oxygen atom.
A) How does the reactivity of neon (atomic number 10, period 2, group 18) differ from that of
sodium (atomic number 11, period 3, group 1)? Explain your reasoning based on the properties
of neon and sodium that you can infer based on their atomic numbers, periods, and groups.
(4 points)
Points
Awarded Criteria
4 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
3 The answer is mostly clear.
The answer is supported by mostly relevant details.
There are a few errors in grammar, usage, or mechanics. Errors do not interfere with
meaning.
2 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
1 The answer is not clear.
There are few or no supporting details.
There are many errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered.
sodium (atomic number 11, period 3, group 1)? Explain your reasoning based on the properties
of neon and sodium that you can infer based on their atomic numbers, periods, and groups.
(4 points)
Points
Awarded Criteria
4 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
3 The answer is mostly clear.
The answer is supported by mostly relevant details.
There are a few errors in grammar, usage, or mechanics. Errors do not interfere with
meaning.
2 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
1 The answer is not clear.
There are few or no supporting details.
There are many errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered.
The reactivity of neon differs significantly from that of sodium due to their positioning on the periodic table. Neon, with an atomic number of 10 and found in Group 18, is a noble gas that possesses a full octet of electrons, making it highly stable and virtually inert; it does not readily form compounds with other elements. In contrast, sodium, with an atomic number of 11 and located in Group 1, has one valence electron, which it readily loses to achieve a stable electron configuration, making sodium highly reactive, particularly with nonmetals like chlorine. Thus, the full electron shell of neon contributes to its lack of reactivity, while the single valence electron of sodium drives its tendency to participate in chemical reactions.
A) The periodic table is arranged by various patterns. Describe the pattern regarding charges
of ions formed across a row? In three to five sentences, explain your reasoning and provide
specific examples. (4 points)
Points
Awarded Criteria
4 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
3 The answer is mostly clear.
The answer is supported by mostly relevant details.
There are a few errors in grammar, usage, or mechanics. Errors do not interfere with
meaning.
2 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
1 The answer is not clear.
There are few or no supporting details.
There are many errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered.
of ions formed across a row? In three to five sentences, explain your reasoning and provide
specific examples. (4 points)
Points
Awarded Criteria
4 The answer is very clear.
The answer is fully supported by details.
There may be a few errors in grammar, usage, or mechanics. Errors do not interfere
with meaning.
3 The answer is mostly clear.
The answer is supported by mostly relevant details.
There are a few errors in grammar, usage, or mechanics. Errors do not interfere with
meaning.
2 The answer is somewhat clear.
Details are weak or not related.
There are some errors in grammar, usage, and mechanics. Errors interfere with
meaning.
1 The answer is not clear.
There are few or no supporting details.
There are many errors in grammar, usage, and mechanics. Errors interfere with
meaning.
0 The question is not answered.
The periodic table exhibits a clear pattern regarding the charges of ions formed across a row, reflecting the number of valence electrons in the outer shell of the elements. Generally, elements in Groups 1 and 2 tend to lose electrons to achieve a full outer shell, resulting in positive charges; for example, sodium (Na) in Group 1 forms a Na⁺ ion by losing one electron, while magnesium (Mg) in Group 2 forms a Mg²⁺ ion by losing two electrons. As you move across a period towards Group 14, elements typically do not form ions; however, from Groups 15 to 17, nonmetals gain electrons to achieve a stable electron configuration, leading to negative charges. For instance, chlorine (Cl) in Group 17 gains one electron to form a Cl⁻ ion, whereas oxygen (O) in Group 16 gains two electrons to become O²⁻. This trend illustrates how the position of an element in the periodic table correlates with its ion formation and charge.
1 answer