Final Quiz - Atomic Structure And Chemical Bonding

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  • 1/15 Questions

    Beryllium (Be) has a charge of +2. Nitrogen (N) has a charge of -3. What's the chemical formula?

    • Be6N4
    • Be3N2
    • Be2N
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Final Quiz - Atomic Structure And Chemical Bonding - Quiz

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  • 2. 

    The electron configuration for the element in Group 13/Group 3, period 3 is 2,8,3.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    The electron configuration for the element in Group 13/Group 3, period 3 is 2,8,3. This means that the element has 2 electrons in the first energy level, 8 electrons in the second energy level, and 3 electrons in the third energy level. This configuration is consistent with the periodic table and the organization of electrons in atoms. Therefore, the statement is true.

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  • 3. 

    What property do metals have that allow them to be hit or shaped without breaking?

    • Conductivity

    • Density

    • Mobility

    • Malleability

    Correct Answer
    A. Malleability
    Explanation
    Metals have the property of malleability, which allows them to be hit or shaped without breaking. Malleability refers to the ability of a material to be easily deformed under compression, such as being hammered or rolled into thin sheets. This property is due to the metallic bonds that hold the atoms together in a metal lattice structure, allowing the atoms to move and slide past each other without causing the material to fracture.

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  • 4. 

    Beryllium has a charge of +2. Fluorine has a charge of -1. What's the chemical formula?

    • Be2F2

    • Be4F8

    • BeF2

    • Be2F

    Correct Answer
    A. BeF2
    Explanation
    Beryllium has a charge of +2 and fluorine has a charge of -1. In order to balance the charges, there needs to be two fluorine atoms for every beryllium atom. Therefore, the correct chemical formula is BeF2.

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  • 5. 

    Element X has 2 electron shells.  The outer shell has 6 electrons.  It is a nonmetal. Which element is Element X?

    • Fluorine

    • Chlorine

    • Carbon

    • Oxygen

    Correct Answer
    A. Oxygen
    Explanation
    Oxygen is the correct answer because it has 2 electron shells, with the outer shell containing 6 electrons. Additionally, oxygen is a nonmetal.

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  • 6. 

    This type of bond is brittle, and only conducts electricity when dissolved. Which bond is it?

    • Metallic Bonding

    • Ionic Bonding

    • Covalent Bonding

    Correct Answer
    A. Ionic Bonding
    Explanation
    Ionic bonding is a type of bond that involves the transfer of electrons from one atom to another, resulting in the formation of oppositely charged ions. These ions are held together by strong electrostatic forces, creating a crystal lattice structure. This type of bond is brittle because the strong forces between ions make it difficult for them to move past one another, causing the crystal to shatter easily. Additionally, ionic compounds only conduct electricity when dissolved in water or melted, as the ions are free to move and carry electric charge.

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  • 7. 

    Silicon has a proton number of 14. State it's electron configuration.

    Correct Answer
    2,8,4
    2, 8, 4
    Explanation
    The electron configuration of an atom represents the distribution of electrons in its energy levels. Silicon has an atomic number of 14, which means it has 14 protons and 14 electrons. The electron configuration of silicon is 2,8,4, which indicates that the first energy level (K shell) has 2 electrons, the second energy level (L shell) has 8 electrons, and the third energy level (M shell) has 4 electrons. The repetition of 2,8,4 after the comma suggests that the electron configuration pattern continues beyond the M shell, but it is not necessary to include it in the answer.

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  • 8. 

    Which group of the periodic table has elements which are extremely reactive and silvery soft?

    • Alkali Metals

    • Noble Gases

    • Alkali Earth Metals

    • Transition Metals

    Correct Answer
    A. Alkali Metals
    Explanation
    Alkali metals are extremely reactive and silvery soft. They have only one valence electron, which makes them highly reactive and prone to losing that electron in chemical reactions. This reactivity increases as you move down the group, with the lower elements being more reactive than the higher ones. Additionally, alkali metals are soft and can be easily cut with a knife due to their low melting and boiling points. Therefore, the group of elements in the periodic table that fits this description is the alkali metals.

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  • 9. 

    Metallic bonds are generally stronger when...

    • There are more electrons in the sea of electrons.

    • There are more neutrons.

    • There are less electrons in the sea of electrons.

    • The metal can conduct electricity.

    Correct Answer
    A. There are more electrons in the sea of electrons.
    Explanation
    Metallic bonds occur when the outer electrons of metal atoms are delocalized and form a "sea" of electrons. These electrons are free to move throughout the metal lattice, creating a strong bond between the metal atoms. Therefore, the more electrons there are in this sea, the stronger the metallic bond will be.

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  • 10. 

    Element N has four isotopes. N-19, N-20, N-21, and N-22.  Out of 100 atoms of the element N, 20 are N-19. 9 are N-20 52 are N-21 19 are N-22 Calculate the relative atomic mass of N.

    Correct Answer
    20.7
    Explanation
    (20x19) + (9x20) + (52x21) + (19x22)
    /100
    = 20.7

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  • 11. 

    The chemical Formaldehyde has a chemical formula of CH2O.  The carbon atom needs and can share 4 electrons. The oxygen atom needs and can share 2 electrons. The hydrogen atoms need and can share 1 electron. State the structure that is true for this bond.

    • The oxygen atom has a single bond with the Carbon atom, and the hydrogen atoms have a double bond with the Carbon atom.

    • The Hydrogen atoms each have a double bond with the Oxygen atom, and the Oxygen atom has a single bond with the Carbon atom.

    • The carbon bond has a single bond with both hydrogen atoms, and a double bond with the oxygen atom.

    • The Carbon atom has a single bond with the Oxygen atom, and the Hydrogen atoms have a single bond with the Oxygen atom.

    Correct Answer
    A. The carbon bond has a single bond with both hydrogen atoms, and a double bond with the oxygen atom.
    Explanation
    http://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/Images/structure1.gif

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  • 12. 

    Vanadium is more reactive than Strontium.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Strontium is more to the left of the periodic table, and in a lower period than Vanadium is.

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  • 13. 

    Uranium has three isotopes. 0.005% is Uranium-234. 0.720% is Uranium-235. 99.275% is Uranium-238. Give the approximate relative atomic mass of Uranium, to four decimal places.

    Correct Answer
    237.9782
    Explanation
    (0.005x234)+(0.720x235)+(99.275x238)
    /100
    = 237.9732

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  • 14. 

    Which property of an element does an isotope change?

    • Reaction rates

    • Malleability

    • Melting point

    • Shininess

    Correct Answer
    A. Melting point
    Explanation
    Isotopes are different forms of an element that have the same number of protons but different numbers of neutrons. The presence of different isotopes can affect the overall mass and stability of an element. Since the melting point of a substance is determined by the strength of the bonds between its atoms, the presence of isotopes with different masses can lead to variations in the strength of these bonds. Therefore, an isotope can change the melting point of an element.

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  • 15. 

    For a nice and easy final question, Which bond has the highest melting points?

    • Covalent

    • Ionic

    • Metallic

    Correct Answer
    A. Metallic
    Explanation
    Metallic bonds have the highest melting points compared to covalent and ionic bonds. This is because metallic bonds involve the sharing of delocalized electrons among a lattice of positively charged metal ions. The strong attraction between the positive ions and the negatively charged electrons requires a significant amount of energy to break the bond and transition from solid to liquid state. In contrast, covalent bonds involve the sharing of electrons between atoms, and ionic bonds involve the transfer of electrons from one atom to another, both of which are generally weaker than metallic bonds.

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  • Aug 29, 2024
    Quiz Edited by
    ProProfs Editorial Team
  • Nov 06, 2011
    Quiz Created by
    Superoxideion01
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