IBSL Chemistry Topic 4 Bonding Multiple Choice Questions

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  • 1/21 Questions

    Which compound contains bith covalent and ionic bonds? Sodium carbonate magnesium bromide dichloromethane ethanoic acid

    • Sodium carbonate
    • Magnesium bromide
    • Dichloromethane
    • Ethanoic acid
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IBSL Chemistry Topic 4 Bonding Multiple Choice Questions - Quiz
About This Quiz

This IBSL Chemistry quiz focuses on Topic 4: Bonding, assessing knowledge through multiple-choice questions. It covers covalent and ionic bonds, electronegativity, and molecular geometry, providing a thorough evaluation of understanding in these areas.

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  • 2. 

    What is the valence shell eectron pair repulsion (VSEPR) Theory used to predict?

    • The energy levels in an atom

    • The shapes of molecules and ions

    • The electronegativities of elements

    • The type of bonding in an compound

    Correct Answer
    A. The shapes of molecules and ions
    Explanation
    The Valence Shell Electron Pair Repulsion (VSEPR) Theory is used to predict the shapes of molecules and ions. This theory states that electron pairs in the valence shell of an atom repel each other and therefore arrange themselves in a way that maximizes the distance between them. By considering the number of electron pairs around the central atom and their repulsion, the VSEPR theory allows us to determine the most likely shape of a molecule or ion. This is important in understanding the properties and behavior of chemical compounds.

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  • 3. 

    Whicn molecule is linear?

    • SO2

    • CO2

    • H2S

    • Cl2O

    Correct Answer
    A. CO2
    Explanation
    CO2 is a linear molecule because it consists of two oxygen atoms bonded to a central carbon atom. The carbon-oxygen double bonds are arranged in a straight line, resulting in a linear molecular shape. The other molecules listed, SO2, H2S, and Cl2O, have a bent or angular shape due to the presence of lone pairs or different atom arrangements.

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  • 4. 

    Which pair of elements is most likely to form a covalently bonded compound?

    • Li and Cl

    • Ca and S

    • P and O

    • Zn and Br

    Correct Answer
    A. P and O
    Explanation
    P and O are most likely to form a covalently bonded compound because both elements have relatively high electronegativity values. Covalent bonding occurs when atoms share electrons, and elements with similar electronegativity values are more likely to share electrons equally. In the case of P and O, both elements have a strong attraction for electrons, making it likely that they will form a covalent bond by sharing electrons between them.

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  • 5. 

    Element X is in Group 2 and element Y is in Group 7, of the periodic table. Which ions will be present in the compound formed when X and Y react together?

    • X+ and Y-

    • X+ and Y-

    • X2+ and Y-

    • X2- and Y+

    Correct Answer
    A. X2+ and Y-
    Explanation
    When element X from Group 2 reacts with element Y from Group 7, they will form an ionic compound. Group 2 elements lose 2 electrons to achieve a stable octet configuration, forming a 2+ cation. Group 7 elements gain 1 electron to achieve a stable octet configuration, forming a 1- anion. Therefore, element X will form X2+ cations and element Y will form Y- anions in the compound formed when they react together.

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  • 6. 

    Given the following electronegativities, which bond would be the most polar? H: 2.2 N: 3.0 O: 3.5 F: 4.0

    • O-H in H2O

    • N-O in NO2

    • N-F in NF2

    • N-H in NH3

    Correct Answer
    A. O-H in H2O
    Explanation
    The bond between O and H in H2O would be the most polar because the electronegativity difference between O and H is the largest compared to the other bond options. Oxygen (O) has an electronegativity of 3.5, while hydrogen (H) has an electronegativity of 2.2. The greater the electronegativity difference between two atoms, the more polar the bond between them becomes. Therefore, the O-H bond in H2O is the most polar.

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  • 7. 

    In which of the following substances would hydrogen bonding be expected to occur?

    • II only

    • I and III only

    • I and II only

    • I, II and III

    Correct Answer
    A. II only
    Explanation
    Hydrogen bonding occurs when hydrogen is bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine. In option II, water (H2O) is present, which contains hydrogen bonded to oxygen atoms. This allows for hydrogen bonding to occur between water molecules. In options I and III, there is no mention of substances that contain hydrogen bonded to highly electronegative atoms, so hydrogen bonding would not be expected to occur. Therefore, the correct answer is II only.

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  • 8. 

    How do bond length and bond strength change as the number of bonds between two atoms increases?

    • Bond length increases and bond strength increases

    • Bond length increases and bond strength decreases

    • Bond length decreases and bond strength increases

    • Bond length decreases and bond strength decreases

    Correct Answer
    A. Bond length decreases and bond strength increases
    Explanation
    As the number of bonds between two atoms increases, the bond length decreases. This is because the atoms are held closer together, resulting in a shorter bond length. Additionally, the bond strength increases because more bonds between atoms require more energy to break them apart. Therefore, the correct answer is that bond length decreases and bond strength increases.

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  • 9. 

    Which statement is true for most ionic compounds?

    • They contain elements of similar electronegativity

    • They conduct electricity in the solid state

    • They are colored

    • They have high melting and boiling point

    Correct Answer
    A. They have high melting and boiling point
    Explanation
    Most ionic compounds have high melting and boiling points because they are held together by strong electrostatic forces of attraction between positively and negatively charged ions. These forces require a significant amount of energy to overcome, resulting in high melting and boiling points.

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  • 10. 

    A solid has a melting point of 1440 degrees celsius. It conducts heat and electricity. It does not dissolve in water or in organic solvents. The bond between the particles is most likely to be

    • Covalent

    • Ionic

    • Dipole:dipole

    • Metallic

    Correct Answer
    A. Metallic
    Explanation
    Based on the given information, the solid conducts heat and electricity, which suggests the presence of delocalized electrons that can move freely within the solid. Additionally, the solid does not dissolve in water or organic solvents, indicating a strong bond between its particles. These characteristics are consistent with metallic bonding, where positively charged metal ions are held together by a sea of delocalized electrons. Therefore, the most likely bond between the particles in this solid is metallic.

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  • 11. 

    Which substance has the lowest electrical conductivity?

    • Cu(s)

    • Hg(l)

    • H2(g)

    • LiOH(aq)

    Correct Answer
    A. H2(g)
    Explanation
    H2(g) has the lowest electrical conductivity because it is a non-metal and does not have any free-moving charged particles. Cu(s) is a metal and has high electrical conductivity due to the presence of delocalized electrons. Hg(l) is also a metal and has relatively high electrical conductivity. LiOH(aq) is an ionic compound that dissociates into Li+ and OH- ions in solution, allowing for the flow of charged particles and therefore higher electrical conductivity than H2(g).

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  • 12. 

    Which of the following is true for CO2?

    • C=O bond is polar and CO2 molecule is non-polar

    • C=O bond is non-polar and CO2 molecule is polar

    • C=O bond is polar and CO2 molecule is polar

    • C=O bond is non-polar and CO2 molecule is non-polar

    Correct Answer
    A. C=O bond is polar and CO2 molecule is non-polar
    Explanation
    CO2 is a linear molecule with two oxygen atoms bonded to a central carbon atom. The electronegativity difference between carbon and oxygen is significant, causing the C=O bond to be polar. However, the molecule as a whole is non-polar due to its symmetrical geometry. The two polar bonds cancel each other out, resulting in a non-polar molecule.

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  • 13. 

    Why is the boiling point of pH3 lower than that of NH3?

    • PH3 is non-polar whereas NH2 is polar

    • PH3 is not hydrogen bonded whereas NH3 is hydrogen bonded

    • Van der Waals' forces are weaker in PH3 than in NH3

    • The molar mass of PH3 is greater than that of NH3

    Correct Answer
    A. PH3 is not hydrogen bonded whereas NH3 is hydrogen bonded
    Explanation
    The boiling point of a substance is determined by the strength of the intermolecular forces between its molecules. Hydrogen bonding is a strong intermolecular force that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is attracted to another electronegative atom in a different molecule. NH3 can form hydrogen bonds between its nitrogen atom and the hydrogen atoms of neighboring NH3 molecules, which increases the strength of the intermolecular forces and raises its boiling point. On the other hand, PH3 does not have hydrogen bonding because phosphorus is less electronegative than nitrogen, resulting in weaker intermolecular forces and a lower boiling point.

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  • 14. 

    When the H-N-H bond angles in the species NH2-, NH3 and NH4+ are arranged in order of increasing bond angle (smallest bond angle first), which order is correct?

    • NH2- < NH3 < NH4+

    • NH4+ < NH3 < NH2-

    • NH3 < NH2- < NH4+

    • NH2- < NH4+ < NH3

    Correct Answer
    A. NH2- < NH3 < NH4+
    Explanation
    The H-N-H bond angles in NH2- are smaller than in NH3 because NH2- has a lone pair of electrons that repel the bonding pairs, causing the bond angle to decrease. NH3 has a larger bond angle than NH2- because it has one less lone pair of electrons, reducing the repulsion between the bonding pairs. NH4+ has the largest bond angle because it has no lone pairs of electrons, resulting in the least repulsion between the bonding pairs. Therefore, the correct order is NH2- < NH3 < NH4+.

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  • 15. 

    When

    • CH4, NH3, H2O

    • NH3, CH4, H2O

    • NH3, H2O, CH4

    • H2O, NH3, CH4

    Correct Answer
    A. H2O, NH3, CH4
    Explanation
    The correct answer is H2O, NH3, CH4. This is because the given compounds are listed in alphabetical order.

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  • 16. 

    When the following bond types are listed in decreasing order of strength (strongest first), what is the correct order?

    • Covalent> Hydrogen>Van der Waals'

    • Covalent> Van der Waals' > Hydrogen

    • Hydrogen>Covalent>Van der Waals'

    • Van der Waals'> Hydrogen> Covalent

    Correct Answer
    A. Covalent> Hydrogen>Van der Waals'
    Explanation
    Covalent bonds are the strongest type of chemical bond, as they involve the sharing of electrons between atoms. Hydrogen bonds are weaker than covalent bonds but still stronger than Van der Waals' forces. Hydrogen bonds occur when a hydrogen atom is attracted to a highly electronegative atom, such as oxygen or nitrogen. Van der Waals' forces are the weakest type of bond and are caused by temporary fluctuations in electron distribution, resulting in temporary positive and negative charges. Therefore, the correct order of bond strength is Covalent> Hydrogen> Van der Waals'.

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  • 17. 

    Which substance is most soluble in water (in mol dm-3) at 298K?

    • CH3CH3

    • CH3OCH3

    • CH3CH2OH

    • CH3CH2CH2CH2OH

    Correct Answer
    A. CH3CH2OH
    Explanation
    CH3CH2OH (ethanol) is the most soluble substance in water at 298K. This is because ethanol can form hydrogen bonds with water molecules through its hydroxyl (-OH) group. The hydroxyl group is polar and can attract the partially positive hydrogen atoms in water, allowing for strong intermolecular attractions and high solubility. In contrast, the other substances listed (CH3CH3, CH3OCH3, and CH3CH2CH2CH2OH) do not have hydroxyl groups and cannot form hydrogen bonds with water to the same extent, resulting in lower solubility.

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  • 18. 

    Which one of the following statement is correct?

    • The energy absorbed when liquid ammonia boils is used to overcome the covalent bond within the ammonia molecule

    • The energy absorbed when solid phosphorus (P4) melts is used to overcome the ionic bonds between the phosphorus molecules

    • The energy absorbed when sodium chloride dissolves in water is used to form ions

    • The energy absorbed when copper metal melts is used to overcome the non-directional metallic bonds between the copper atoms

    Correct Answer
    A. The energy absorbed when copper metal melts is used to overcome the non-directional metallic bonds between the copper atoms
    Explanation
    The energy absorbed when copper metal melts is used to overcome the non-directional metallic bonds between the copper atoms. Metallic bonds are formed between metal atoms, where the valence electrons are delocalized and free to move throughout the structure. When copper metal melts, the energy absorbed is used to break these metallic bonds, allowing the copper atoms to move freely and take on a liquid form. This is different from the other options, which involve breaking covalent, ionic, or forming ionic bonds.

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  • 19. 

    Which molecule is non-polar?

    • H2CO

    • SO3

    • NF3

    • CHCl3

    Correct Answer
    A. SO3
    Explanation
    SO3 is a non-polar molecule because it consists of three oxygen atoms bonded to a central sulfur atom. The sulfur-oxygen bonds are polar due to the difference in electronegativity between sulfur and oxygen. However, the molecule is trigonal planar in shape, with the oxygen atoms arranged symmetrically around the sulfur atom. This arrangement cancels out the dipole moments of the polar bonds, resulting in a molecule with no overall dipole moment and therefore non-polar.

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  • 20. 

    In which of the following pairs does the second substance have the lower boiling point?

    • F2, Cl2

    • C2H6, C3H8

    • H2O, H2S

    • CH3OCHE, CH3CH2OH

    Correct Answer
    A. C2H6, C3H8
    Explanation
    The boiling point of a substance is determined by the strength of the intermolecular forces between its molecules. In the given options, C2H6 (ethane) and C3H8 (propane) are both hydrocarbons, but C3H8 has a higher molecular weight and therefore stronger intermolecular forces. Since stronger forces require more energy to break and reach the boiling point, C3H8 has a higher boiling point than C2H6. Therefore, the second substance (C3H8) has a higher boiling point than the first substance (C2H6).

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  • 21. 

    The molar masses of C2H6, CH3OH and CH3F are very similar. How do theur boiling points compare?

    • C2H

    • CH3F

    • CH3OH

    • C2H6

    Correct Answer
    A. C2H6
    Explanation
    The boiling point of a substance is determined by the strength of intermolecular forces between its molecules. In the given options, C2H6 (ethane) has the highest molar mass, which means it has the most number of electrons and a larger surface area compared to the other compounds. This results in stronger London dispersion forces between its molecules, leading to a higher boiling point. Therefore, the boiling point of C2H6 is expected to be higher compared to CH3F (fluoromethane) and CH3OH (methanol).

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  • Mar 22, 2023
    Quiz Edited by
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  • Nov 05, 2012
    Quiz Created by
    Ssamreth

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