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Questions and Answers
An element has an atomic number of 16. Which ion will it most likely form to achieve a stable electron configuration?
An element has an atomic number of 16. Which ion will it most likely form to achieve a stable electron configuration?
- X⁻¹
- X⁺²
- X⁻² (correct)
- X⁺¹
Why do ionic compounds typically exhibit high melting and boiling points?
Why do ionic compounds typically exhibit high melting and boiling points?
- The ions are highly mobile and easily separated at room temperature.
- They consist of discrete molecules with weak intermolecular forces.
- The electrostatic forces between ions are strong and require significant energy to overcome. (correct)
- They form metallic bonds, which are strong but easily disrupted by thermal energy.
Which molecular geometry results from a central atom bonded to three other atoms with one lone pair of electrons?
Which molecular geometry results from a central atom bonded to three other atoms with one lone pair of electrons?
- Bent
- Tetrahedral
- Trigonal planar
- Trigonal pyramidal (correct)
In which of the following molecules would you expect the bond angle to be closest to 120°?
In which of the following molecules would you expect the bond angle to be closest to 120°?
Sodium chloride (NaCl) is a poor conductor of electricity in its solid state but conducts electricity when molten. What explains this difference in conductivity?
Sodium chloride (NaCl) is a poor conductor of electricity in its solid state but conducts electricity when molten. What explains this difference in conductivity?
Which property is generally observed in substances with strong metallic bonding?
Which property is generally observed in substances with strong metallic bonding?
Magnesium chloride (MgCl₂) generally possesses a higher melting point compared to NaCl. Which factor primarily accounts for this difference?
Magnesium chloride (MgCl₂) generally possesses a higher melting point compared to NaCl. Which factor primarily accounts for this difference?
Water (H₂O) has a higher boiling point than hydrogen sulfide (H₂S). Which intermolecular force is primarily responsible for this difference?
Water (H₂O) has a higher boiling point than hydrogen sulfide (H₂S). Which intermolecular force is primarily responsible for this difference?
What type of intermolecular force is primarily responsible for the relatively high boiling point of water (H₂O)?
What type of intermolecular force is primarily responsible for the relatively high boiling point of water (H₂O)?
Metals like aluminum are excellent conductors of electricity. Which statement best explains how metals conduct electricity?
Metals like aluminum are excellent conductors of electricity. Which statement best explains how metals conduct electricity?
Which of the following compounds is least likely to exhibit significant electrical conductivity in the solid state?
Which of the following compounds is least likely to exhibit significant electrical conductivity in the solid state?
What happens to the shared electrons in a covalent bond if one of the atoms is significantly more electronegative than the other?
What happens to the shared electrons in a covalent bond if one of the atoms is significantly more electronegative than the other?
Which type of bond requires the most energy to break, given similar molecular sizes?
Which type of bond requires the most energy to break, given similar molecular sizes?
Flashcards
Ionic Bonding
Ionic Bonding
Electrostatic attraction between oppositely charged ions, forming a lattice structure. Example: Sodium Chloride (NaCl).
High Melting/Boiling Points in Ionic Compounds
High Melting/Boiling Points in Ionic Compounds
High melting and boiling points are due to strong electrostatic forces between ions, which require significant energy to overcome.
Conductivity of NaCl
Conductivity of NaCl
Solid NaCl has ions in fixed positions, so it cannot conduct electricity; molten NaCl has mobile ions which can carry a charge.
Polar Covalent Bond
Polar Covalent Bond
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Electrical Conductivity in Metals
Electrical Conductivity in Metals
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Electron Configuration
Electron Configuration
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Ion
Ion
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Molecular Shape
Molecular Shape
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Bond Angle
Bond Angle
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Metallic Bonding
Metallic Bonding
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Intermolecular Forces
Intermolecular Forces
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Giant Ionic Lattice
Giant Ionic Lattice
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Covalent Bond
Covalent Bond
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Study Notes
- The document is a Chemical Bonding Test for the Access to Medicine & Medical Biosciences program.
- Time allowed for the test is 1 hour 15 minutes.
- Instructions state to answer all questions, write answers in the provided spaces, and use the periodic table.
Multiple Choice Questions - Section A
- The ground state electron configuration for oxygen (atomic number 8) is 1s² 2s² 2p⁴.
- Oxygen will form an ion with a 2- charge.
- Carbon dioxide (CO2) has a linear shape.
- A molecule with a tetrahedral shape, like methane (CH4), has a bond angle of approximately 109.5°.
- High electrical conductivity is a property associated with metallic bonding.
- London dispersion forces best describe the intermolecular forces present in iodine (I2).
- Sodium chloride (NaCl) has a giant ionic lattice structure.
- In covalent bonding, electrons are shared between atoms.
- Ionic compounds are conductive when dissolved in water.
- A molecule of nitrogen (N2) has a triple covalent bond.
Short Answer Questions - Section B
- Task is to write the electron configuration for the chloride ion (Cl-).
- Task is to describe the shape of an ammonia molecule (NH3) and explain its bond angles, including drawing a dot and cross diagram.
- Task is to define ionic bonding and provide an example of a compound formed through ionic bonding.
- Task is to explain why ionic compounds generally have high melting and boiling points.
- Task is to explain why sodium chloride (NaCl) does not conduct electricity in its solid state but does in molten states.
- Task is to explain why magnesium chloride (MgCl2) has a higher melting point than NaCl.
- Task is to define a polar covalent bond and provide an example of a molecule with a polar covalent bond.
- Task is to explain why water (H2O) has a higher boiling point than hydrogen sulfide (H2S), referencing the types of intermolecular forces present.
- Task is to explain the increase in boiling point from H2S to H2Te.
- Task is to use a diagram to explain how metals such as aluminum are able to conduct electricity.
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Description
Chemical bonding test for medicine and biosciences programs. Questions cover electron configuration, ion formation, molecular shapes, types of bonding, intermolecular forces, and conductivity. Includes multiple choice and short answer questions.
