A bond formed by the complete transfer of electrons from one atom to another is

Answer: Ionic Ionic bonds form between low-electronegativity (metal) and high-electronegativity (nonmetal) atoms — electrons transfer to create cations and anions.

A covalent bond between two identical atoms (e.g., H-H) is

Answer: Nonpolar (electrons shared equally) Same atoms have the same electronegativity → equal sharing → nonpolar covalent.

The H-Cl bond is best described as

Answer: Polar covalent (Cl pulls electrons more strongly) Cl is more electronegative than H, so the shared electron pair spends more time near Cl, giving partial charges (δ⁻ on Cl, δ⁺ on H).

AP Chemistry · Topic 2.1

Types of Chemical Bonds Practice

Part of Compound Structure and Properties.(SAP-3.A)

Practice questions

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Sample questions

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Sample 1difficulty 1/5
$A bond formed by the complete transfer of electrons from one atom to another is$
- A
  $Ionic$
  check_circle
- B
  $Covalent$
- C
  $Hydrogen bond$
- D
  $Metallic$
Why
$Ionic bonds form between low-electronegativity (metal) and high-electronegativity (nonmetal) atoms — electrons transfer to create cations and anions.$
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Sample 2difficulty 2/5
$A covalent bond between two identical atoms (e.g., H-H) is$
- A
  $Nonpolar (electrons shared equally)$
  check_circle
- B
  $Polar$
- C
  $Metallic$
- D
  $Ionic$
Why
$Same atoms have the same electronegativity \to equal sharing \to nonpolar covalent.$
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Sample 3difficulty 2/5
$The H-Cl bond is best described as$
- A
  $Polar covalent (Cl pulls electrons more strongly)$
  check_circle
- B
  $Metallic$
- C
  $Pure ionic$
- D
  $Nonpolar covalent$
Why
$Cl is more electronegative than H, so the shared electron pair spends more time near Cl, giving partial charges (δ⁻ on Cl, δ⁺ on H).$
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Sample 4difficulty 3/5
$Which bond is most polar?$
- A
  $O-H$
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- B
  $C-H$
- C
  $All are equally polar$
- D
  $N-H$
Why
$O-H has the largest electronegativity difference (1.4), making it the most polar of the three.$
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Sample 5difficulty 3/5
$Two diagrams contrast NaCl (Na+ and Cl- ions) with Cl2 (two chlorine atoms sharing a bonding pair of electrons).$
$Which best distinguishes ionic from covalent bonding?$
- A
  $Ionic bonds form between ions (large EN difference); covalent bonds share electrons (small EN difference)$
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- B
  $Ionic bonds are weaker than covalent bonds$
- C
  $Ionic bonds are always polar covalent$
- D
  $Covalent bonds only form between metals$
Why
$A large electronegativity difference (>~1.7) drives complete electron transfer (ionic), whereas similar electronegativities lead to electron sharing (covalent).$
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