A Unique Quiz On Bonding Period 5
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The quiz below is derived from chapter 4.2 and is the fifth in a series of quizzes designed to test out how much of it you understood. Take it up and see if you have adequate knowledge on bonding periods. All the best and remember the more you practice the more information you get to retain.
Questions and Answers
- 1.
Bond of oppositely charged ions
- A.
Covalent bond
- B.
Ionic bond
- C.
Metallic bond
Correct Answer
B. Ionic bondExplanation
An ionic bond is formed when oppositely charged ions are attracted to each other. In this type of bond, one atom donates electrons to another atom, resulting in the formation of positive and negative ions. These ions are held together by electrostatic forces of attraction, creating a strong bond. Ionic bonds are typically formed between metals and nonmetals, where the metal atom loses electrons to become a positive ion, and the nonmetal atom gains those electrons to become a negative ion. This transfer of electrons creates a stable and balanced compound.Rate this question:
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- 2.
Bond between positively charged nucleus of one atom and the negatively charged electron cloud of another atom
- A.
Covalent bond
- B.
Ionic bond
- C.
Metallic bond
- D.
Polyatomic ion
Correct Answer
C. Metallic bondExplanation
A metallic bond is formed when positively charged metal ions are surrounded by a sea of delocalized electrons. In this type of bond, the positively charged nucleus of one atom is attracted to the negatively charged electron cloud of another atom, creating a strong bond. This allows for the sharing and movement of electrons between atoms, resulting in the unique properties of metals such as high electrical and thermal conductivity, malleability, and ductility.Rate this question:
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- 3.
Bond formed whem two atoms share electrons
- A.
Covalent bond
- B.
Ionic bond
- C.
Metallic bond
- D.
Polyatomic ion
Correct Answer
A. Covalent bondExplanation
A covalent bond is formed when two atoms share electrons. In this type of bond, the atoms involved have similar electronegativities, meaning they have a similar ability to attract electrons. This allows them to share electrons and form a stable bond. Covalent bonds are typically formed between nonmetal atoms.Rate this question:
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- 4.
When two or more atoms covalently bond and act as a single ion
- A.
Covalent bond
- B.
Ionic bond
- C.
Metallic bond
- D.
Polyatomic ion
Correct Answer
D. Polyatomic ionExplanation
A polyatomic ion is a group of two or more atoms that are covalently bonded together but act as a single charged particle. This means that they have a net positive or negative charge and can participate in ionic bonding with other ions. Unlike covalent or metallic bonds, which involve the sharing or pooling of electrons between atoms, a polyatomic ion retains its molecular structure and behaves as a single unit. Therefore, the given answer "polyatomic ion" is the correct choice for the described scenario.Rate this question:
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- 5.
Why do some atoms join to form bonds?
- A.
They have magnetive fields
- B.
To get a full outer shell of valence electrons
- C.
To be like BOND....JAMES BOND
- D.
Their chemical properties are always alike so they need to bond
Correct Answer
B. To get a full outer shell of valence electronsExplanation
Atoms join to form bonds in order to achieve a full outer shell of valence electrons. The outermost shell of an atom, known as the valence shell, is responsible for the atom's chemical reactivity. By forming bonds, atoms can share, gain, or lose electrons to achieve a stable electron configuration, typically with eight electrons in the valence shell. This stability is achieved by following the octet rule, which states that atoms tend to gain, lose, or share electrons to attain a configuration similar to the noble gases.Rate this question:
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- 6.
The alkali metalls have how many valence electrons?
- A.
4
- B.
3
- C.
2
- D.
1
Correct Answer
D. 1Explanation
The alkali metals have one valence electron. Valence electrons are the electrons in the outermost energy level of an atom, and they are responsible for the chemical properties of an element. The alkali metals are found in Group 1 of the periodic table, and they all have one valence electron. This electron is easily lost, making the alkali metals highly reactive and able to form strong bonds with other elements.Rate this question:
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- 7.
Alkali metals will likely form this type of bond
- A.
Ionic
- B.
Covalent
- C.
Metallic
Correct Answer
A. IonicExplanation
Alkali metals, such as lithium, sodium, and potassium, have one electron in their outermost energy level. They tend to lose this electron to achieve a stable electron configuration, resulting in a positive ion. Other elements, typically non-metals, readily gain this electron to achieve a stable configuration, forming a negative ion. The attraction between these oppositely charged ions leads to the formation of ionic bonds. Therefore, alkali metals are more likely to form ionic bonds.Rate this question:
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- 8.
Which family does this element belong?
- A.
Alkali Metals
- B.
Noble Gases
- C.
Halogens
- D.
Transition Metals
Correct Answer
C. HalogensExplanation
Halogens are a group of highly reactive elements found in Group 17 of the periodic table. They include elements such as fluorine, chlorine, bromine, iodine, and astatine. These elements have seven valence electrons and are known for their ability to form salts. They have a strong tendency to gain or share one electron to achieve a stable electron configuration. Therefore, the element in question belongs to the Halogens family.Rate this question:
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- 9.
How many valence electrons does this element have?
- A.
17
- B.
7
- C.
35
- D.
18
Correct Answer
B. 7Explanation
The element in question has 7 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom and are involved in chemical reactions. The atomic number of the element is 17, which indicates that it has 17 electrons. To determine the number of valence electrons, we look at the electron configuration of the element. The element with atomic number 17 is chlorine (Cl), and its electron configuration is 2-8-7. The outermost energy level contains 7 electrons, which are the valence electrons.Rate this question:
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- 10.
What type of bond is this?
- A.
Ionic
- B.
Covalent
- C.
Metallic
Correct Answer
B. CovalentExplanation
This bond is covalent because covalent bonds involve the sharing of electrons between atoms. In this type of bond, electrons are shared between two nonmetal atoms, resulting in the formation of a stable molecule. Ionic bonds involve the transfer of electrons from one atom to another, while metallic bonds involve a sea of delocalized electrons surrounding a lattice of positive ions.Rate this question:
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- 11.
What type of bond is this?
- A.
Polar covalent
- B.
Nonpolar covalent
- C.
Metallic
- D.
Ionic
Correct Answer
B. Nonpolar covalentExplanation
This bond is a nonpolar covalent bond because it involves the sharing of electrons between two atoms with similar electronegativities. In a nonpolar covalent bond, the electrons are shared equally between the atoms, resulting in a balanced distribution of charge.Rate this question:
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- 12.
What type of bond is this?
- A.
Polar covalent
- B.
Nonpolar covalent
- C.
Metallic
- D.
Ionic
Correct Answer
A. Polar covalentExplanation
This bond is likely a polar covalent bond because it involves the sharing of electrons between atoms of different electronegativities. In a polar covalent bond, one atom has a higher electronegativity than the other, resulting in an uneven distribution of electron density. As a result, there is a partial positive charge on one atom and a partial negative charge on the other. This creates a dipole moment and gives the bond its polar nature.Rate this question:
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- 13.
Which element has the the highest electron affinity?
- A.
Li
- B.
F
- C.
Si
- D.
C
Correct Answer
B. FExplanation
Fluorine (F) has the highest electron affinity among the given elements. Electron affinity refers to the amount of energy released when an atom gains an electron. Fluorine has a high electron affinity because it has a small atomic radius and a high effective nuclear charge, making it highly attractive to electrons. Additionally, fluorine only needs to gain one electron to achieve a stable electron configuration, which further increases its electron affinity.Rate this question:
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- 14.
Electron Affinity is important for....
- A.
Polar covalent bonds
- B.
Nonpolar covalent bonds
Correct Answer
A. Polar covalent bondsExplanation
Electron affinity is important for polar covalent bonds because it measures the energy change that occurs when an atom gains an electron. In polar covalent bonds, electrons are shared unequally between atoms, resulting in a partial positive and partial negative charge. The electron affinity of an atom determines how strongly it attracts and holds onto electrons, which is crucial in forming and stabilizing polar covalent bonds.Rate this question:
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- 15.
What type of bond does this show?
- A.
Ionic
- B.
Covalent
- C.
Metallic
- D.
No bonding is in this picture
Correct Answer
C. MetallicExplanation
This picture shows metallic bonding. Metallic bonding occurs when metal atoms share their valence electrons with a sea of delocalized electrons, creating a "sea of electrons" that holds the metal atoms together. This type of bonding is typically found in metals, such as the one depicted in the picture.Rate this question:
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- 16.
Polyatomic ions can bond to each other?
- A.
Yes
- B.
No
Correct Answer
A. YesExplanation
Polyatomic ions can bond to each other because they are made up of multiple atoms that are covalently bonded together. These ions have a charge and can form ionic bonds with other ions or molecules. When polyatomic ions bond to each other, they create compounds known as polyatomic molecules or polyatomic salts. This bonding allows for the formation of various chemical compounds and plays a crucial role in many chemical reactions and processes.Rate this question:
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- 17.
What type of bonds do polyatomic ions have
- A.
Polar covalent
- B.
Nonpolar covalent
Correct Answer
A. Polar covalentExplanation
Polyatomic ions are formed when a group of atoms gain or lose electrons, resulting in a charged particle. These ions have a specific arrangement of atoms and can have polar covalent bonds. In a polar covalent bond, the electrons are not shared equally between the atoms, resulting in a partial positive charge on one atom and a partial negative charge on the other. This unequal sharing of electrons creates a polarity in the bond. Therefore, polyatomic ions can have polar covalent bonds due to the unequal distribution of electrons between the atoms in the ion.Rate this question:
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- 18.
Which of the following will conduct electricity when dissolved in water?
- A.
Ionic bonds
- B.
Covelent bonds
- C.
Polar covalent bonds
- D.
BOTH polar and nonpolar covalent bonds
Correct Answer
A. Ionic bondsExplanation
Ionic bonds will conduct electricity when dissolved in water because they involve the transfer of electrons from one atom to another, creating ions with positive and negative charges. These charged particles, called ions, are free to move in the solution and carry an electric current. In contrast, covalent bonds involve the sharing of electrons between atoms and do not create ions. Therefore, substances with ionic bonds, such as salts, can conduct electricity in water, while substances with covalent bonds, such as most organic compounds, cannot.Rate this question:
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- 19.
Which of the following is the anion?
- A.
Na
- B.
Cl
Correct Answer
B. ClExplanation
The anion is the negatively charged ion in a compound. In this case, the only option that is an anion is Cl. Na is a cation, which is a positively charged ion.Rate this question:
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- 20.
Which of the following molecules have a higher melting point?
- A.
NaCl
- B.
CO2
Correct Answer
A. NaClExplanation
NaCl has a higher melting point compared to CO2 because it is an ionic compound, while CO2 is a covalent compound. Ionic compounds have strong electrostatic forces of attraction between oppositely charged ions, which require more energy to break and therefore have higher melting points. In contrast, covalent compounds have weaker intermolecular forces, resulting in lower melting points. Therefore, NaCl has a higher melting point than CO2.Rate this question:
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Apr 16, 2024Quiz Edited by
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Jan 24, 2011Quiz Created by
Chip_brand
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