Types of Chemical Bonds - AP Chemistry

Identify the bond type in CH₄.

Covalent bond. Carbon shares electrons equally with four hydrogen atoms.
What type of bond is present in NH₃?

Polar covalent bond. Nitrogen is more electronegative than hydrogen.
Which type of bond is present in H₂O?

Covalent bond. Oxygen and hydrogen share electrons to form the molecule.
Which bond type generally has low melting points, ionic or covalent?

Covalent bond. Weaker intermolecular forces require less energy to overcome.
What is the bond angle in a trigonal planar molecule?

$120^\circ$ . Three atoms arranged in a flat triangle around a central atom.
What is the bond angle in a linear molecule?

$180^\circ$ . Two atoms bonded in a straight line configuration.
What is the bond angle in a tetrahedral molecule?

$109.5^\circ$ . Four atoms arranged around a central atom in 3D space.
What is lattice energy?

The energy required to separate a mole of an ionic solid into gaseous ions. Higher lattice energy indicates stronger ionic bonding.
How does electronegativity difference affect bond type?

Larger differences typically lead to ionic bonds; smaller to covalent. Generally, differences $>1.7$ are ionic, $<0.4$ are nonpolar covalent.
Define a nonpolar covalent bond.

A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.
Which type of bond is present in H₂O?

Covalent bond. Oxygen and hydrogen share electrons to form the molecule.
What is the duet rule?

Hydrogen and Helium achieve stability with 2 valence electrons. Applies because they only need to fill the 1s orbital.
What is the octet rule?

Atoms tend to form bonds until they are surrounded by 8 valence electrons. Applies to most main group elements except hydrogen and helium.
What is the duet rule?

Hydrogen and Helium achieve stability with 2 valence electrons. Applies because they only need to fill the 1s orbital.
What is an example of a molecule with a nonpolar covalent bond?

Methane (CH₄). Carbon and hydrogen have similar electronegativity values.
What is the bond angle in a trigonal planar molecule?

$120^\circ$ . Three atoms arranged in a flat triangle around a central atom.
Identify the bond type in KBr.

Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.
What is the primary force in metallic bonding?

Attraction between free electrons and metal ions. Enables electrical conductivity in metals.
Which type of bond is present in NaCl?

Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.
Which type of bond is present in H₂O?

Covalent bond. Oxygen and hydrogen share electrons to form the molecule.
What is an example of a molecule with a polar covalent bond?

Water (H₂O). Oxygen is more electronegative than hydrogen.
What is the bond angle in a tetrahedral molecule?

$109.5^\circ$ . Four atoms arranged around a central atom in 3D space.
Which bond type is typically the strongest: single, double, or triple covalent bonds?

Triple covalent bond. More electron pairs shared means stronger attraction.
Define a nonpolar covalent bond.

A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.
What is a covalent bond?

A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.
What is the bond angle in a linear molecule?

$180^\circ$ . Two atoms bonded in a straight line configuration.
What is a covalent bond?

A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.
Which bond type allows for electrical conductivity in solid state?

Metallic bond. Mobile electrons can carry electric current.
What is bond length in covalent bonds?

The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.
What type of bond is expected in a compound with high melting point?

Ionic bond. Strong ionic attractions require high temperatures to overcome.
Identify the bond type in Fe.

Metallic bond. Iron atoms share electrons in a metallic lattice.
What is bond length in covalent bonds?

The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.
Identify the bond type in Cl₂.

Nonpolar covalent bond. Two identical chlorine atoms share electrons equally.
Which bond type allows for electrical conductivity when dissolved in water?

Ionic bond. Dissociated ions can move and conduct electricity in solution.
What type of bond is expected in a compound with high melting point?

Ionic bond. Strong ionic attractions require high temperatures to overcome.
Which bond type generally has low melting points, ionic or covalent?

Covalent bond. Weaker intermolecular forces require less energy to overcome.
Identify the bond type in CH₄.

Covalent bond. Carbon shares electrons equally with four hydrogen atoms.
What type of bond is likely in a compound with high conductivity?

Metallic bond. Mobile electrons enable current flow in the solid state.
Which bond type allows for electrical conductivity in solid state?

Metallic bond. Mobile electrons can carry electric current.
Identify the bond type in Fe.

Metallic bond. Iron atoms share electrons in a metallic lattice.
What type of bond is found in metals?

Metallic bond. Allows metals to conduct electricity and be malleable.
Which bond type is typically the longest: single, double, or triple covalent bonds?

Single covalent bond. Fewer electron pairs allow atoms to be farther apart.
What is a coordinate covalent bond?

A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.
What is the primary force in metallic bonding?

Attraction between free electrons and metal ions. Enables electrical conductivity in metals.
What is a covalent bond?

A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.
Which bond type generally has high melting points, ionic or covalent?

Ionic bond. Strong electrostatic forces require more energy to break.
What is bond energy in covalent bonds?

The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.
What is an example of a molecule with a polar covalent bond?

Water (H₂O). Oxygen is more electronegative than hydrogen.
Which bond type is typically the strongest: single, double, or triple covalent bonds?

Triple covalent bond. More electron pairs shared means stronger attraction.
Identify the bond type in CO₂.

Covalent bond. Carbon and oxygen share electrons in double bonds.
What is an example of a molecule with a nonpolar covalent bond?

Methane (CH₄). Carbon and hydrogen have similar electronegativity values.
What type of bond is likely in a compound with high conductivity?

Metallic bond. Mobile electrons enable current flow in the solid state.
What type of bond is present in O₂?

Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.
Identify the bond type in MgO.

Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.
Why do ionic compounds form crystal lattices?

To maximize attraction and minimize repulsion between ions. Optimizes electrostatic interactions in three dimensions.
What is a coordinate covalent bond?

A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.
What is bond energy in covalent bonds?

The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.
Identify the bond type in Cl₂.

Nonpolar covalent bond. Two identical chlorine atoms share electrons equally.
What type of bond is present in NH₃?

Polar covalent bond. Nitrogen is more electronegative than hydrogen.
What type of bond is present in O₂?

Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.
What type of bond is expected in a compound with high melting point?

Ionic bond. Strong ionic attractions require high temperatures to overcome.
What is an ionic bond?

A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.
What is a metallic bond?

A bond involving the attraction between free electrons and positively charged metal ions. Creates a 'sea of electrons' that can move freely throughout the metal structure.
What type of bond is present in O₂?

Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.
Which bond type generally has high melting points, ionic or covalent?

Ionic bond. Strong electrostatic forces require more energy to break.
Which bond type allows for electrical conductivity when dissolved in water?

Ionic bond. Dissociated ions can move and conduct electricity in solution.
What is the octet rule?

Atoms tend to form bonds until they are surrounded by 8 valence electrons. Applies to most main group elements except hydrogen and helium.
What is the primary force in covalent bonding?

Sharing of electron pairs. Allows atoms to achieve stable electron configurations.
Which type of bond is present in NaCl?

Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.
What is lattice energy?

The energy required to separate a mole of an ionic solid into gaseous ions. Higher lattice energy indicates stronger ionic bonding.
What is the bond angle in a linear molecule?

$180^\circ$ . Two atoms bonded in a straight line configuration.
What is a coordinate covalent bond?

A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.
What is the primary force in metallic bonding?

Attraction between free electrons and metal ions. Enables electrical conductivity in metals.
Why do ionic compounds form crystal lattices?

To maximize attraction and minimize repulsion between ions. Optimizes electrostatic interactions in three dimensions.
What is bond energy in covalent bonds?

The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.
Which bond type generally has high melting points, ionic or covalent?

Ionic bond. Strong electrostatic forces require more energy to break.
Define a polar covalent bond.

A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.
What is the primary force in ionic bonding?

Electrostatic attraction. Opposite charges attract according to Coulomb's law.
Identify the bond type in CH₄.

Covalent bond. Carbon shares electrons equally with four hydrogen atoms.
What is the bond angle in a trigonal planar molecule?

$120^\circ$ . Three atoms arranged in a flat triangle around a central atom.
Identify the bond type in CO₂.

Covalent bond. Carbon and oxygen share electrons in double bonds.
What is the primary force in covalent bonding?

Sharing of electron pairs. Allows atoms to achieve stable electron configurations.
What is an example of a molecule with a polar covalent bond?

Water (H₂O). Oxygen is more electronegative than hydrogen.
What is the primary force in ionic bonding?

Electrostatic attraction. Opposite charges attract according to Coulomb's law.
Define a polar covalent bond.

A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.
Which bond type generally has low melting points, ionic or covalent?

Covalent bond. Weaker intermolecular forces require less energy to overcome.
What is an ionic bond?

A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.
Identify the bond type in KBr.

Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.
Which bond type is typically the longest: single, double, or triple covalent bonds?

Single covalent bond. Fewer electron pairs allow atoms to be farther apart.
What is bond length in covalent bonds?

The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.
How does electronegativity difference affect bond type?

Larger differences typically lead to ionic bonds; smaller to covalent. Generally, differences $>1.7$ are ionic, $<0.4$ are nonpolar covalent.
Define a nonpolar covalent bond.

A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.
What is an ionic bond?

A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.
Identify the bond type in MgO.

Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.
Identify the bond type in MgO.

Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.
Identify the bond type in KBr.

Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.
What is the primary force in covalent bonding?

Sharing of electron pairs. Allows atoms to achieve stable electron configurations.
What type of bond is present in NH₃?

Polar covalent bond. Nitrogen is more electronegative than hydrogen.
Identify the bond type in CO₂.

Covalent bond. Carbon and oxygen share electrons in double bonds.
Define a polar covalent bond.

A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.
What type of bond is found in metals?

Metallic bond. Allows metals to conduct electricity and be malleable.
What type of bond is likely in a compound with high conductivity?

Metallic bond. Mobile electrons enable current flow in the solid state.
What is the primary force in ionic bonding?

Electrostatic attraction. Opposite charges attract according to Coulomb's law.
Which type of bond is present in NaCl?

Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.
What is lattice energy?

The energy required to separate a mole of an ionic solid into gaseous ions. Higher lattice energy indicates stronger ionic bonding.

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