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NY Regents Chemistry Chemical Bonding and Molecular Geometry — practice questions

Explore 25 free Chemical Bonding and Molecular Geometry questions in NY Regents Chemistry Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Bonding and Molecular Geometry questions and exercises with answers

Showing questions 1–25 of 25.

A neutral atom loses two electrons from its valence shell. What has it become?Read the answer and worked solution →What force holds the ions of a salt crystal together?Read the answer and worked solution →How much energy is needed to pull one mole of solid sodium chloride apart into gaseous ions?Read the answer and worked solution →A calcium atom loses both of its valence electrons. Its 18 remaining electrons match which noble gas?Read the answer and worked solution →Aluminum sits in group 13 of the periodic table. What charge does its common cation carry?Read the answer and worked solution →Iron has the ground state configuration [Ar]3d6 4s2. Which electrons leave first when the Fe2+ ion forms?Read the answer and worked solution →Two atoms have very similar tendencies to attract electrons. Which bond do they form with each other?Read the answer and worked solution →How do the melting points of covalent compounds compare with those of ionic compounds?Read the answer and worked solution →Two hydrogen atoms approach each other and form a bond. What fixes the bond length?Read the answer and worked solution →In a chlorine molecule the two bonded atoms are identical. How are the bonding electrons shared?Read the answer and worked solution →In a molecule of hydrogen chloride, which atom carries the partial negative charge?Read the answer and worked solution →Which element attracts the electrons in its bonds more strongly than any other element?Read the answer and worked solution →A bond forms between a metal atom and a nonmetal atom. What character does that bond usually have?Read the answer and worked solution →Potassium nitrate is built from K+ ions and NO3- ions. Which bond types are present in the solid?Read the answer and worked solution →Hydrogen does not obey the octet rule. How many electrons fill its valence shell?Read the answer and worked solution →Two atoms share two pairs of electrons between them. What is that bond called?Read the answer and worked solution →You are drawing a Lewis structure for a molecule with several atoms. Which atom normally goes in the center?Read the answer and worked solution →Nitric oxide has 11 valence electrons in total. What does that odd count tell you before you draw anything?Read the answer and worked solution →How does a carbon to carbon triple bond compare with a carbon to carbon single bond?Read the answer and worked solution →Breaking all four carbon to hydrogen bonds in one mole of methane takes 1660 kJ. What is the average bond energy?Read the answer and worked solution →Ammonia has three bonds and one lone pair around its nitrogen atom. What is the shape of the molecule?Read the answer and worked solution →Carbon dioxide contains two polar carbon to oxygen bonds, yet the whole molecule is nonpolar. Why?Read the answer and worked solution →Swap to line up one familyRead the answer and worked solution →Drop each formula by bond typeRead the answer and worked solution →Swipe each molecule by polarityRead the answer and worked solution →

Worked practice questions

A neutral atom loses two electrons from its valence shell. What has it become?

  1. A cation carrying a 2+ charge
  2. An anion carrying a 2- charge
  3. An isotope with added mass
  4. A radical with a lone electron
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Correct answer: A. A cation carrying a 2+ charge

1. Losing electrons leaves the particle with more protons than electrons, so it ends up positive. 2. A positive ion is a cation, and every electron lost adds one unit of positive charge. 3. Two electrons lost therefore leave a cation with a 2+ charge. 4. Gaining electrons would instead make an anion, so the negative option does not fit. _Source: OpenStax Chemistry (CC BY 4.0), Chs 7 and 17, section 7.1 Ionic Bonding_

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What force holds the ions of a salt crystal together?

  1. Equal sharing of one pair of electrons
  2. Overlap of two half filled orbitals
  3. Electrostatic attraction between opposite charges
  4. Weak attraction between neutral molecules
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Correct answer: C. Electrostatic attraction between opposite charges

1. A salt is built from cations, which are positive, and anions, which are negative. 2. Opposite charges pull on each other, and that pull is an electrostatic force. 3. This electrostatic attraction between cations and anions is the ionic bond itself. 4. Sharing electrons would make a covalent bond instead, which is a different mechanism. _Source: OpenStax Chemistry (CC BY 4.0), Chs 7 and 17, section 7.1 Ionic Bonding_

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How much energy is needed to pull one mole of solid sodium chloride apart into gaseous ions?

  1. 436 kJ
  2. 769 kJ
  3. 243 kJ
  4. 185 kJ
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Correct answer: B. 769 kJ

1. Separating the lattice means overcoming every attraction between the ions at once. 2. For one mole of solid sodium chloride that costs 769 kilojoules. 3. The other values belong to covalent bonds, which are far weaker than a whole ionic lattice. _Source: OpenStax Chemistry (CC BY 4.0), Chs 7 and 17, section 7.1 Ionic Bonding_

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