Ions And Ionic Bonding
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Questions and Answers
- 1.
During bonding, atoms try to gain a ____ valence shell
Explanation
During bonding, atoms try to gain a full valence shell. This is because a full valence shell is the most stable configuration for an atom. By gaining or losing electrons, atoms can achieve a full valence shell and become more stable. This stability is achieved by following the octet rule, where atoms strive to have 8 electrons in their outermost shell, except for hydrogen and helium which strive to have 2 electrons. By gaining a full valence shell, atoms can achieve a lower energy state and increase their stability.Rate this question:
- 2.
Select the 3 ways atoms can bond
- A.
Ionic bond
- B.
Covalent bond
- C.
Metallic bond
Correct Answer(s)
A. Ionic bond
B. Covalent bond
C. Metallic bondExplanation
Atoms can bond in three ways: ionic bond, covalent bond, and metallic bond. In an ionic bond, atoms transfer electrons to achieve a stable electron configuration. This results in the formation of positively and negatively charged ions that are attracted to each other. In a covalent bond, atoms share electrons to fill their outermost electron shells. This sharing of electrons creates a strong bond between the atoms. In a metallic bond, electrons are delocalized and free to move within a lattice of positively charged metal ions. This results in a strong bond between the metal atoms.Rate this question:
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- 3.
A metal and non-metal bond. The metal wants to give badly, the non-metal wants to take badly. The metal gives the non metal an electron. The metal is now a postitive cation and the non-metal is a negative anion. Since they are opposite charges, they attract. What bond is this?
- A.
Ionic bond
- B.
Covalent bond
- C.
Metallic bond
- D.
Technically, its none of the above
Correct Answer
A. Ionic bondExplanation
This is an ionic bond because it involves the transfer of electrons from a metal to a non-metal. The metal, which wants to give electrons, becomes a positive cation, while the non-metal, which wants to take electrons, becomes a negative anion. The opposite charges of the cation and anion attract each other, forming an ionic bond.Rate this question:
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- 4.
What's a lattice?
- A.
A green, edible leaf found on burgers and in salads
- B.
An arrangement of cations and anions attracted to each other
- C.
A huge structure
- D.
A skyscraper
Correct Answer
B. An arrangement of cations and anions attracted to each otherExplanation
The correct answer is an arrangement of cations and anions attracted to each other. A lattice refers to a regular, repeating pattern of positive and negative ions in a crystal structure. In a lattice, cations (positively charged ions) and anions (negatively charged ions) are arranged in a way that their opposite charges attract each other, creating a stable and organized structure. This arrangement is commonly found in ionic compounds, where the strong electrostatic forces between the ions hold them together in a lattice formation.Rate this question:
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- 5.
Study this image. The magnesium gave 2 electrons, and became a _____ with a ___ charge
- A.
Cation, +2
- B.
Cation, -2
- C.
Anion, +2
- D.
Anion, -2
Correct Answer
A. Cation, +2Explanation
When magnesium gives away 2 electrons, it loses those negatively charged particles, resulting in a positively charged ion. This type of ion is called a cation. The charge on the cation is determined by the number of electrons lost, which in this case is 2, so the charge is +2.Rate this question:
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- 6.
Calcuate Li^(+) (NO_3)^(-)
Correct Answer
Li (NO_3)Explanation
The given answer, Li (NO_3), represents a lithium ion (Li+) combined with a nitrate ion (NO3-). This compound is formed when a lithium atom loses one electron to become a positively charged ion (Li+), and a nitrate ion (NO3-) donates its negative charge to combine with the lithium ion. The resulting compound is Li (NO3), where the lithium ion and nitrate ion are held together by ionic bonds.Rate this question:
- 7.
The atoms above are sharing electrons to imitate a full valence shell. What is this an example of?
- A.
Ionic bond
- B.
Covalent bond
- C.
Metallic bond
- D.
Technically, its none of the above
Correct Answer
B. Covalent bondExplanation
This is an example of a covalent bond because in a covalent bond, atoms share electrons to achieve a full valence shell.Rate this question:
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- 8.
Generally, halogens such as oxygen (O) and fluorine (F) hang around in pairs, (O_2) and (F_2) due to a covalent bond.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
Halogens such as oxygen and fluorine exist as diatomic molecules, meaning they naturally occur as pairs of atoms bonded together. This is because they have a high electronegativity, which allows them to form strong covalent bonds with each other. Therefore, the statement that halogens hang around in pairs is true.Rate this question:
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- 9.
Let's find out what Al + O_2 is. The Al ion has a ___ charge. The O_2 ion has a ___ charge. Thus, when we combine them, we get
- A.
2-, 3+, Al_2 O_3
- B.
3+, 2-, Al_3 O_2
- C.
3+, 2-, Al_2 O_3
- D.
2-, 3+, Al_3 O_2
Correct Answer
C. 3+, 2-, Al_2 O_3Explanation
The Al ion has a 3+ charge because it is a metal and tends to lose electrons to form positive ions. The O2- ion has a 2- charge because oxygen tends to gain two electrons to achieve a stable octet configuration. When we combine these ions, we need two Al3+ ions to balance the charge of three O2- ions, resulting in the formula Al2O3.Rate this question:
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- 10.
Unfortunately, Al + O_2 --> Al_2 O_3 makes no sense because it isn't balanced. Balance it
Correct Answer
4Al + 3O_2 --> 2(Al_2 O_3)Explanation
The given equation, 4Al + 3O_2 --> 2(Al_2 O_3), is the balanced form of the chemical equation Al + O_2 --> Al_2 O_3. In order for a chemical equation to be balanced, the number of atoms of each element on both sides of the equation must be equal. The balanced equation shows that there are 4 atoms of aluminum (Al) and 6 atoms of oxygen (O) on both sides of the equation, satisfying the law of conservation of mass.Rate this question:
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Mar 21, 2023Quiz Edited by
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Feb 28, 2016Quiz Created by
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