AP Chemistry Flashcards: Types Of Chemical Bonds

What this deck covers

This deck focuses on Types Of Chemical Bonds, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: Identify the bond type in CH₄.

Answer: Covalent bond. Carbon shares electrons equally with four hydrogen atoms.

Flashcard 2: What type of bond is present in NH₃?

Answer: Polar covalent bond. Nitrogen is more electronegative than hydrogen.

Flashcard 3: Which type of bond is present in H₂O?

Answer: Covalent bond. Oxygen and hydrogen share electrons to form the molecule.

Flashcard 4: Which bond type generally has low melting points, ionic or covalent?

Answer: Covalent bond. Weaker intermolecular forces require less energy to overcome.

Flashcard 5: What is the bond angle in a trigonal planar molecule?

Answer: $120^\circ$. Three atoms arranged in a flat triangle around a central atom.

Flashcard 6: What is the bond angle in a linear molecule?

Answer: $180^\circ$. Two atoms bonded in a straight line configuration.

Flashcard 7: What is the bond angle in a tetrahedral molecule?

Answer: $109.5^\circ$. Four atoms arranged around a central atom in 3D space.

Flashcard 8: What is lattice energy?

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

Flashcard 9: How does electronegativity difference affect bond type?

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

Flashcard 10: Define a nonpolar covalent bond.

Answer: A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.

Flashcard 11: Which type of bond is present in H₂O?

Answer: Covalent bond. Oxygen and hydrogen share electrons to form the molecule.

Flashcard 12: What is the duet rule?

Answer: Hydrogen and Helium achieve stability with 2 valence electrons. Applies because they only need to fill the 1s orbital.

Flashcard 13: What is the octet rule?

Answer: Atoms tend to form bonds until they are surrounded by 8 valence electrons. Applies to most main group elements except hydrogen and helium.

Flashcard 14: What is the duet rule?

Answer: Hydrogen and Helium achieve stability with 2 valence electrons. Applies because they only need to fill the 1s orbital.

Flashcard 15: What is an example of a molecule with a nonpolar covalent bond?

Answer: Methane (CH₄). Carbon and hydrogen have similar electronegativity values.

Flashcard 16: What is the bond angle in a trigonal planar molecule?

Answer: $120^\circ$. Three atoms arranged in a flat triangle around a central atom.

Flashcard 17: Identify the bond type in KBr.

Answer: Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.

Flashcard 18: What is the primary force in metallic bonding?

Answer: Attraction between free electrons and metal ions. Enables electrical conductivity in metals.

Flashcard 19: Which type of bond is present in NaCl?

Answer: Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.

Flashcard 20: Which type of bond is present in H₂O?

Answer: Covalent bond. Oxygen and hydrogen share electrons to form the molecule.

Flashcard 21: What is an example of a molecule with a polar covalent bond?

Answer: Water (H₂O). Oxygen is more electronegative than hydrogen.

Flashcard 22: What is the bond angle in a tetrahedral molecule?

Answer: $109.5^\circ$. Four atoms arranged around a central atom in 3D space.

Flashcard 23: Which bond type is typically the strongest: single, double, or triple covalent bonds?

Answer: Triple covalent bond. More electron pairs shared means stronger attraction.

Flashcard 24: Define a nonpolar covalent bond.

Answer: A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.

Flashcard 25: What is a covalent bond?

Answer: A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.

Flashcard 26: What is the bond angle in a linear molecule?

Answer: $180^\circ$. Two atoms bonded in a straight line configuration.

Flashcard 27: What is a covalent bond?

Answer: A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.

Flashcard 28: Which bond type allows for electrical conductivity in solid state?

Answer: Metallic bond. Mobile electrons can carry electric current.

Flashcard 29: What is bond length in covalent bonds?

Answer: The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.

Flashcard 30: What type of bond is expected in a compound with high melting point?

Answer: Ionic bond. Strong ionic attractions require high temperatures to overcome.

Flashcard 31: Identify the bond type in Fe.

Answer: Metallic bond. Iron atoms share electrons in a metallic lattice.

Flashcard 32: What is bond length in covalent bonds?

Answer: The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.

Flashcard 33: Identify the bond type in Cl₂.

Answer: Nonpolar covalent bond. Two identical chlorine atoms share electrons equally.

Flashcard 34: Which bond type allows for electrical conductivity when dissolved in water?

Answer: Ionic bond. Dissociated ions can move and conduct electricity in solution.

Flashcard 35: What type of bond is expected in a compound with high melting point?

Answer: Ionic bond. Strong ionic attractions require high temperatures to overcome.

Flashcard 36: Which bond type generally has low melting points, ionic or covalent?

Answer: Covalent bond. Weaker intermolecular forces require less energy to overcome.

Flashcard 37: Identify the bond type in CH₄.

Answer: Covalent bond. Carbon shares electrons equally with four hydrogen atoms.

Flashcard 38: What type of bond is likely in a compound with high conductivity?

Answer: Metallic bond. Mobile electrons enable current flow in the solid state.

Flashcard 39: Which bond type allows for electrical conductivity in solid state?

Answer: Metallic bond. Mobile electrons can carry electric current.

Flashcard 40: Identify the bond type in Fe.

Answer: Metallic bond. Iron atoms share electrons in a metallic lattice.

Flashcard 41: What type of bond is found in metals?

Answer: Metallic bond. Allows metals to conduct electricity and be malleable.

Flashcard 42: Which bond type is typically the longest: single, double, or triple covalent bonds?

Answer: Single covalent bond. Fewer electron pairs allow atoms to be farther apart.

Flashcard 43: What is a coordinate covalent bond?

Answer: A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.

Flashcard 44: What is the primary force in metallic bonding?

Answer: Attraction between free electrons and metal ions. Enables electrical conductivity in metals.

Flashcard 45: What is a covalent bond?

Answer: A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.

Flashcard 46: Which bond type generally has high melting points, ionic or covalent?

Answer: Ionic bond. Strong electrostatic forces require more energy to break.

Flashcard 47: What is bond energy in covalent bonds?

Answer: The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.

Flashcard 48: What is an example of a molecule with a polar covalent bond?

Answer: Water (H₂O). Oxygen is more electronegative than hydrogen.

Flashcard 49: Which bond type is typically the strongest: single, double, or triple covalent bonds?

Answer: Triple covalent bond. More electron pairs shared means stronger attraction.

Flashcard 50: Identify the bond type in CO₂.

Answer: Covalent bond. Carbon and oxygen share electrons in double bonds.

Flashcard 51: What is an example of a molecule with a nonpolar covalent bond?

Answer: Methane (CH₄). Carbon and hydrogen have similar electronegativity values.

Flashcard 52: What type of bond is likely in a compound with high conductivity?

Answer: Metallic bond. Mobile electrons enable current flow in the solid state.

Flashcard 53: What type of bond is present in O₂?

Answer: Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.

Flashcard 54: Identify the bond type in MgO.

Answer: Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.

Flashcard 55: Why do ionic compounds form crystal lattices?

Answer: To maximize attraction and minimize repulsion between ions. Optimizes electrostatic interactions in three dimensions.

Flashcard 56: What is a coordinate covalent bond?

Answer: A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.

Flashcard 57: What is bond energy in covalent bonds?

Answer: The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.

Flashcard 58: Identify the bond type in Cl₂.

Answer: Nonpolar covalent bond. Two identical chlorine atoms share electrons equally.

Flashcard 59: What type of bond is present in NH₃?

Answer: Polar covalent bond. Nitrogen is more electronegative than hydrogen.

Flashcard 60: What type of bond is present in O₂?

Answer: Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.

Flashcard 61: What type of bond is expected in a compound with high melting point?

Answer: Ionic bond. Strong ionic attractions require high temperatures to overcome.

Flashcard 62: What is an ionic bond?

Answer: A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.

Flashcard 63: What is a metallic bond?

Answer: 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.

Flashcard 64: What type of bond is present in O₂?

Answer: Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.

Flashcard 65: Which bond type generally has high melting points, ionic or covalent?

Answer: Ionic bond. Strong electrostatic forces require more energy to break.

Flashcard 66: Which bond type allows for electrical conductivity when dissolved in water?

Answer: Ionic bond. Dissociated ions can move and conduct electricity in solution.

Flashcard 67: What is the octet rule?

Answer: Atoms tend to form bonds until they are surrounded by 8 valence electrons. Applies to most main group elements except hydrogen and helium.

Flashcard 68: What is the primary force in covalent bonding?

Answer: Sharing of electron pairs. Allows atoms to achieve stable electron configurations.

Flashcard 69: Which type of bond is present in NaCl?

Answer: Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.

Flashcard 70: What is lattice energy?

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

Flashcard 71: What is the bond angle in a linear molecule?

Answer: $180^\circ$. Two atoms bonded in a straight line configuration.

Flashcard 72: What is a coordinate covalent bond?

Answer: A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.

Flashcard 73: What is the primary force in metallic bonding?

Answer: Attraction between free electrons and metal ions. Enables electrical conductivity in metals.

Flashcard 74: Why do ionic compounds form crystal lattices?

Answer: To maximize attraction and minimize repulsion between ions. Optimizes electrostatic interactions in three dimensions.

Flashcard 75: What is bond energy in covalent bonds?

Answer: The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.

Flashcard 76: Which bond type generally has high melting points, ionic or covalent?

Answer: Ionic bond. Strong electrostatic forces require more energy to break.

Flashcard 77: Define a polar covalent bond.

Answer: A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.

Flashcard 78: What is the primary force in ionic bonding?

Answer: Electrostatic attraction. Opposite charges attract according to Coulomb's law.

Flashcard 79: Identify the bond type in CH₄.

Answer: Covalent bond. Carbon shares electrons equally with four hydrogen atoms.

Flashcard 80: What is the bond angle in a trigonal planar molecule?

Answer: $120^\circ$. Three atoms arranged in a flat triangle around a central atom.

Flashcard 81: Identify the bond type in CO₂.

Answer: Covalent bond. Carbon and oxygen share electrons in double bonds.

Flashcard 82: What is the primary force in covalent bonding?

Answer: Sharing of electron pairs. Allows atoms to achieve stable electron configurations.

Flashcard 83: What is an example of a molecule with a polar covalent bond?

Answer: Water (H₂O). Oxygen is more electronegative than hydrogen.

Flashcard 84: What is the primary force in ionic bonding?

Answer: Electrostatic attraction. Opposite charges attract according to Coulomb's law.

Flashcard 85: Define a polar covalent bond.

Answer: A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.

Flashcard 86: Which bond type generally has low melting points, ionic or covalent?

Answer: Covalent bond. Weaker intermolecular forces require less energy to overcome.

Flashcard 87: What is an ionic bond?

Answer: A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.

Flashcard 88: Identify the bond type in KBr.

Answer: Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.

Flashcard 89: Which bond type is typically the longest: single, double, or triple covalent bonds?

Answer: Single covalent bond. Fewer electron pairs allow atoms to be farther apart.

Flashcard 90: What is bond length in covalent bonds?

Answer: The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.

Flashcard 91: How does electronegativity difference affect bond type?

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

Flashcard 92: Define a nonpolar covalent bond.

Answer: A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.

Flashcard 93: What is an ionic bond?

Answer: A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.

Flashcard 94: Identify the bond type in MgO.

Answer: Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.

Flashcard 95: Identify the bond type in MgO.

Answer: Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.

Flashcard 96: Identify the bond type in KBr.

Answer: Ionic bond. $K^+$ and $Br^-$ ions form through electron transfer.

Flashcard 97: What is the primary force in covalent bonding?

Answer: Sharing of electron pairs. Allows atoms to achieve stable electron configurations.

Flashcard 98: What type of bond is present in NH₃?

Answer: Polar covalent bond. Nitrogen is more electronegative than hydrogen.

Flashcard 99: Identify the bond type in CO₂.

Answer: Covalent bond. Carbon and oxygen share electrons in double bonds.

Flashcard 100: Define a polar covalent bond.

Answer: A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.