The Ultimate Bonding Period Quiz 1
A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. The ultimate bonding period quiz one below is designed to help you see just how much you understood the topic on bonds. Give it a try and get to polish your skills!
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 a bond formed between oppositely charged ions. In this type of bond, one atom loses electrons to become positively charged (cation), while another atom gains those electrons to become negatively charged (anion). The attraction between these opposite charges holds the ions together, creating a strong bond. Ionic bonds typically occur between a metal and a non-metal, where the metal donates electrons to the non-metal. This results in the formation of a stable 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 there is a strong attraction between the positively charged nucleus of one atom and the negatively charged electron cloud of another atom. In metallic bonding, the valence electrons are delocalized and can move freely throughout the metal lattice, creating a "sea" of electrons. This allows for the conductivity of electricity and heat in metals. Therefore, metallic bond is the correct answer in this case.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 electrons are shared between the atoms, resulting in a stable arrangement of electrons for both atoms. This sharing of electrons allows both atoms to achieve a full outer electron shell, similar to the noble gases. Covalent bonds are typically formed between nonmetallic elements and can result in the formation of molecules.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
When two or more atoms covalently bond and act as a single ion, they form a polyatomic ion. A polyatomic ion is a charged particle that consists of two or more atoms held together by covalent bonds. Unlike individual atoms, polyatomic ions have an overall charge due to the gain or loss of electrons. These ions can exist independently and participate in chemical reactions, often forming compounds with other ions or molecules. Examples of polyatomic ions include ammonium (NH4+), sulfate (SO42-), and carbonate (CO32-).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 stable electron configuration, specifically to have a full outer shell of valence electrons. This is because atoms are more stable when their outermost energy level is complete. By sharing, gaining, or losing electrons, atoms can achieve a full outer shell and become more stable. This stability is crucial for atoms to form chemical compounds and participate in various chemical reactions.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. In the case of alkali metals, they have one electron in their outermost energy level, which makes them highly reactive and eager to lose that electron to form a positive ion.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 sodium and potassium, are highly reactive elements that have one valence electron. To achieve a stable electron configuration, they tend to lose this electron and form a positive ion. On the other hand, non-metals, such as oxygen and chlorine, have a high affinity for electrons and tend to gain electrons to form negative ions. When alkali metals react with non-metals, such as halogens, they transfer their valence electron to the non-metal, resulting in the formation of ions with opposite charges. This electrostatic attraction between the positive and negative ions leads to the formation of ionic bonds. Therefore, alkali metals are 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
This element belongs to the Halogens family. Halogens are a group of highly reactive nonmetals that are located in Group 17 of the periodic table. They include elements like fluorine, chlorine, bromine, iodine, and astatine. These elements have seven valence electrons and tend to gain one electron to achieve a stable electron configuration. They are known for their high electronegativity and ability to form salts with metals.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
C. 35Explanation
The element with atomic number 35 is bromine (Br). Bromine belongs to Group 17 or the halogen group in the periodic table. Elements in this group have 7 valence electrons. Therefore, the correct answer is 35.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 likely covalent because covalent bonds involve the sharing of electrons between atoms. In an ionic bond, electrons are transferred from one atom to another, while in a metallic bond, electrons are delocalized and shared among a sea of atoms. Since the question does not provide any specific information about the nature of the bond, covalent is the most reasonable choice as it is the most common type of bond formed between nonmetals.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 that have similar electronegativity values. In a nonpolar covalent bond, the electrons are shared equally between the atoms, resulting in a balanced distribution of charge. This type of bond is typically formed between two nonmetals.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
A polar covalent bond is formed when two atoms share electrons unequally, resulting in a slight positive charge on one atom and a slight negative charge on the other. In this type of bond, the electronegativity difference between the atoms is significant, causing the electrons to be pulled closer to the more electronegative atom. This creates a partial positive charge on one end of the bond and a partial negative charge on the other end. The given answer, polar covalent, suggests that the bond being described is formed between two atoms with different electronegativities, resulting in an unequal sharing of electrons.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 is the energy change that occurs when an electron is added to a neutral atom to form a negative ion. Fluorine has a strong attraction for electrons due to its high electronegativity and small atomic size, making it highly favorable for it to gain an electron. This results in a large release of energy, indicating a high electron affinity for fluorine compared to the other elements listed.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 refers to the energy change that occurs when an atom gains an electron. In polar covalent bonds, atoms with higher electron affinity have a stronger attraction for electrons, resulting in an unequal sharing of electrons between atoms. This unequal sharing creates a partial positive charge on one atom and a partial negative charge on the other, leading to the formation of polar covalent bonds. Therefore, understanding the electron affinity of atoms is crucial in determining the polarity of 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
The type of bond shown in the picture is metallic. This is because metallic bonds occur between metal atoms, where the outermost electrons are delocalized and shared among all the atoms in the metallic structure. This allows for the formation of a lattice of positive metal ions surrounded by a "sea" of delocalized electrons. This type of bonding is typically found in metals, which have high electrical and thermal conductivity, malleability, and ductility.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 composed of multiple atoms that are covalently bonded together. These ions can form ionic compounds by transferring or sharing electrons with other ions. The attraction between the positive and negative charges of the ions allows them to bond together and create stable compounds. Therefore, it is possible for polyatomic ions to bond to each other.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 made up of multiple atoms bonded together by covalent bonds. In a polar covalent bond, the electrons are shared unequally between the atoms, resulting in a slight positive charge on one atom and a slight negative charge on the other. This uneven distribution of charge creates a polarity in the bond. Since polyatomic ions are composed of polar covalent bonds, they also possess a net dipole moment, making them polar in nature.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 ions can move freely in the water, allowing the flow of electric current. In contrast, covalent bonds, whether polar or nonpolar, involve the sharing of electrons and do not create charged ions, so they do not conduct electricity when dissolved in water.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, Na is a cation because it is a positively charged ion, while Cl is an anion because it is a negatively 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 positively and negatively charged ions, which require more energy to break and melt the compound. In contrast, covalent compounds have weaker intermolecular forces, such as London dispersion forces, which are easier to overcome, resulting in a lower melting point.Rate this question:
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Current Version
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Mar 19, 2023Quiz Edited by
ProProfs Editorial Team -
Jan 24, 2011Quiz Created by
Chip_brand
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