Chemical Bonding

What type of bonding does NaCl have?
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic
Which of the following is in an ionic bond?
1. MgCl₂
2. H₂O
3. NO
4. F₂
What type of bond exists in NO?
1. polar covalent
2. non-polar covalent
3. ionic
4. metallic
Which of the following contains a nonpolar covalent bond?
1. H₂O
2. MgO
3. F₂
4. NaCl
When a metal forms an ionic bond with a non-metal, the nonmetal atoms will _____.
1. lose and electron and become a negative ion
2. gain an electron and become a negative ion
3. lose an electron and become a positive ion
4. gain an electron and become a positive ion
A bond in which electrons are shared equally is known as _____.
1. ionic
2. polar covalent
3. non-polar covalent
4. metallic
The type of bond that involves a cation and an anion is _____.
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic
Of the following, the most likely pair to form an ionic bond is _____.
1. a halogen and an alkaline earth metal
2. an alkaline earth metal and a transition element
3. an alkali metal and an alkaline earth metal
4. a halogen and a mettalloid
Which of the following differences in electronegativity is most likely to result in the formation of an ionic bond?
1. less than zero
2. between zero and 0.3
3. between 0.3 and 1.7
4. greater than 1.7
Which of the following contains a covalent bond?
1. NO₃
2. NaCl
3. Li₂O
4. Mg₃N₂
The energy released in the formation of an ionic compound is known as _____.
1. lattice energy
2. thermal energy
3. start-up energy
4. ionization energy
The model for metallic bonding is known as _____.
1. the electron sea model
2. the Rutherford model
3. the electron cloud model
4. the quantum model
Which of the following is NOT a property of a metal?
1. low electronegativity
2. may be solid, liquid, or gas at room temperature
3. shiny
4. low ionization energy
The relative numbers of atoms of each kind in any chemical compound (using atomic symbols and subscripts) is known as a _____.
1. chemical formula
2. molecular formula
3. compound formula
4. scientific formula
Which of the following cannot be represented by a molecular formula?
1. an ionic compound
2. a molecular compound
3. a covalent compound
4. a polar compound
The less the electronegativity differences between two bonded atoms, the greater the _____.
1. covalent character
2. ionic character
3. metallic character
4. polar character
H₂O is _____.
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic
In a crystalline compound, each anion is surrounded by _____.
1. positive ions
2. negaitive ions
3. dipoles
4. molecules
The melting points of molecular compounds are usually _____.
1. equal to those of ionic compounds
2. higher than those of ionic compound
3. lower than those of ionic compounds
4. below zero
A substance that can easily be cut into sections is known as _____.
1. sectile
2. docile
3. sessile
4. brittle
When a covalent bond is formed, the potential energy is_____.
1. at a minimum
2. at a maximum
3. at zero
4. equal to the kinetic energy
Which type of bonding would be expected between H and F?
1. ionic
2. non-polar covalent
3. polar covalent
4. hydraulic
Which type of bonding would be expected between Cu and S?
1. ionic
2. non-polar covalent
3. polar covalent
4. hydraulic
Which type of bonding would be expected between I and Br?
1. ionic
2. non-polar covalent
3. polar covalent
4. hydraulic
Which type of bonding would be expected between S and Cs?
1. ionic
2. non-polar covalent
3. polar covalent
4. complex
Which type of bonding would be expected between S and Cl?
1. ionic
2. non-polar covalent
3. polar covalent
4. polyionic
Which type of bonding would be expected between Cl and Br?
1. ionic
2. non-polar covalent
3. polar covalent
4. static
Which of the following describes an ionic compound?
1. low melting point
2. high melting point
3. low boiling point
4. easily vaporize
A charged group of covalently bonded atoms is known as a _____.
1. polyatomic ion
2. polyionic molecule
3. molecular ionic compound
4. ionic molecule
Atoms bond primarily to _____.
1. reduce their potential energy and gain stability
2. increase their potential energy and gain stability
3. make more atoms
4. increase thier potential energy and lose stability
Polar refers to _____.
1. bonds that have an uneven distribution of charge
2. bonds that have an even distribution of charge
3. the formation of uneven size ions
4. even-sized electronegativities in a bond
Which is true of a non-polar covalent bond?
1. the electron pair is shared equally by the bonded atoms
2. the electron pair is shared unequally by the bonded atoms
3. the electronegativity difference of the atoms is very large
4. the electron affinity difference of the atoms is very large
Molecules usually involve which type of atoms?
1. two nonmetals
2. two metals
3. one metal and one nonmetal
4. group 1 elements and group 17 elements
What determines bond length?
1. the distance at which potential energy is at a minimum
2. the point at which the attraction forces outweighs the repulsion forces
3. the distance at whch potential energy is at a maximum
4. the distance at which the two atoms are as close as possible
How are bond length and bond energies related?
1. the higher the bond energy, the shorter the bond length
2. the lower the bond energy, the shorter the bond length
3. the higher the bond energy, the longer the bond length
4. they are not related
What is the general relationship between lattice energy and ionic bond strength?
1. the greater the lattice energy, the stronger the ionic bond
2. the greater the lattice energy, the weaker the ionic bond
3. the weaker the lattice energy, the stronger the ionic bond
4. there is no relationship
Which is the primary reason the properties of ionic and molecular compounds differ?
1. the difference in how strongly the compound's basic units are held together
2. the difference in the strength of the bond between the atoms making up the compound
3. the difference in electron affinity
4. the difference in ionization energy
Polyatomic ions combine with ions of opposite charge to form _____.
1. ionic compounds
2. molecules
3. covalent compounds
4. charged particles
Mobile electrons within bonding networks best describes which type of bond?
1. metallic
2. polar covalent
3. nonpolar covalent
4. ionic
Which type of bond would result in a good conductor of electricity when the substance is dissolved in an aqueous solution?
1. ionic
2. polar covalent
3. nonpolar covalent
4. metallic

Chemical Bonding - 1

Multiple-Choice Exercise
Content © 2006 Melanie Cecere; Authors of Activity: Melanie Cecere & Tami Maloney; All rights reserved. No commercial, for-profit use of this material is allowed. E-mail comments and questions to Tami Maloney.

Chemical Bonding - 1

Multiple-Choice ExerciseContent © 2006 Melanie Cecere; Authors of Activity: Melanie Cecere & Tami Maloney; All rights reserved. No commercial, for-profit use of this material is allowed. E-mail comments and questions to Tami Maloney.

Multiple-Choice Exercise
Content © 2006 Melanie Cecere; Authors of Activity: Melanie Cecere & Tami Maloney; All rights reserved. No commercial, for-profit use of this material is allowed. E-mail comments and questions to Tami Maloney.