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Quizzes > Science

NH2OH Lewis Structure Quiz

Quick quiz to test your H2NOH Lewis structure skills. Instant results.

Editorial: Review CompletedCreated By: Tonesha LandersUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art molecules and quiz text showing Lewis structure H2NOH and key chemical bonds on sky blue background

Use this quiz to master the NH2OH Lewis structure by counting valence electrons, placing single bonds, and checking lone pairs and formal charges. You will get instant feedback on each step, plus tips if a bond or charge is off. When you want more practice, explore molecular geometry practice and deepen your understanding with intermolecular forces in ch3oh.

How many total valence electrons are present in the Lewis structure of H2NOH (hydroxylamine)?
16
14
12
10
Count the valence electrons: each H contributes 1 (3 H's = 3), N contributes 5, and O contributes 6, for a total of 14 valence electrons. This total guides the placement of bonds and lone pairs in the Lewis structure. .
Which atom serves as the central atom in the Lewis structure of H2NOH?
Hydrogen
Oxygen
Both N and O equally
Nitrogen
Nitrogen is the least electronegative atom (other than hydrogen) and can form three bonds, making it the natural central atom for binding to H, H, and O. Hydrogen never serves as a central atom in simple molecules. .
How many lone pairs of electrons are on the nitrogen atom in the Lewis structure of H2NOH?
3
0
2
1
Nitrogen contributes 5 valence electrons. After forming three sigma bonds (two N - H and one N - O), two electrons remain as one lone pair on the nitrogen atom. .
How many lone pairs of electrons are on the oxygen atom in the Lewis structure of H2NOH?
3
0
2
1
Oxygen brings 6 valence electrons; after forming one sigma bond with nitrogen and one with hydrogen, four electrons remain as two lone pairs. .
What is the formal charge on the nitrogen atom in the most stable Lewis structure of H2NOH?
0
+1
+2
-1
Formal charge is calculated as valence electrons minus (nonbonding electrons + half bonding electrons). For nitrogen: 5 - (2 nonbonding + ½·6 bonding) = 0. .
What is the formal charge on the oxygen atom in the most stable Lewis structure of H2NOH?
+2
0
+1
-1
For oxygen: 6 - (4 nonbonding + ½·4 bonding) = 0, so the formal charge is zero. This distribution yields a more stable Lewis structure. .
What is the molecular geometry around the nitrogen atom in H2NOH according to VSEPR theory?
Tetrahedral
Bent
Trigonal planar
Trigonal pyramidal
Nitrogen has three bonded atoms and one lone pair (four electron domains), which by VSEPR gives a trigonal pyramidal molecular shape. .
Approximately what is the H - N - O bond angle in the Lewis structure of H2NOH?
90°
107°
104.5°
109.5°
With one lone pair on nitrogen, the ideal tetrahedral angle (109.5°) is reduced slightly due to lone pair repulsion, giving approximately 107°. .
What is the hybridization of the nitrogen atom in H2NOH?
dsp3
sp
sp2
sp3
Nitrogen has four electron domains (three bonds + one lone pair), corresponding to sp3 hybridization. .
What is the hybridization of the oxygen atom in the hydroxyl group of H2NOH?
sp
sp3
sp2
dsp3
Oxygen has four electron domains (two bonds + two lone pairs), which correspond to sp3 hybridization. .
Approximately what is the bond length of the N - O single bond in H2NOH?
1.35 Å
1.60 Å
1.25 Å
1.45 Å
Typical N - O single bond lengths are around 1.45 Å. This value arises from the overlap of sp3 orbitals on both atoms. .
How many sigma (?) bonds are present in H2NOH?
5
2
3
4
H2NOH has two N - H ? bonds, one N - O ? bond, and one O - H ? bond, totaling four ? bonds. .
How many pi (?) bonds are present in the Lewis structure of H2NOH?
3
1
0
2
All bonds in H2NOH are single ? bonds. There are no multiple bonds, so there are zero ? bonds. .
Is the molecule H2NOH polar or nonpolar?
Depends on conformation
Only polar at low temperature
Nonpolar
Polar
Hydroxylamine is polar due to the electronegativity difference between N/O and H, and its asymmetric shape yields a nonzero dipole moment. .
What is the electron-pair geometry around the oxygen atom in H2NOH?
Trigonal planar
Trigonal pyramidal
Tetrahedral
Linear
Oxygen has four electron domains (two bonds and two lone pairs), which correspond to a tetrahedral electron-pair geometry. .
What is the oxidation state of nitrogen in H2NOH?
+1
+2
0
-1
Assign H as +1 each (3 H's = +3) and O as - 2: let x be N's oxidation state. x +3 + ( - 2) = 0, so x = - 1. .
Which type of intermolecular force is most significant for pure H2NOH?
Hydrogen bonding
London dispersion forces
Ion-dipole interactions
Dipole-dipole interactions
Hydroxylamine has N - H and O - H bonds capable of hydrogen bonding, which dominate its intermolecular interactions. .
Which atom's lone pair constitutes the highest occupied molecular orbital (HOMO) in H2NOH?
Oxygen lone pair
Nitrogen lone pair
O - H ? bond
N - H ? bond
Oxygen is more electronegative, so its nonbonding lone pair lies highest in energy (HOMO) relative to other nonbonding orbitals. .
What is the bond order of the N - O bond in H2NOH?
1.5
0.5
1
2
The N - O bond is a single ? bond without any ? bonding, giving it a bond order of 1. .
Which X - H bond in H2NOH has the higher bond dissociation energy (BDE)?
O - H bond
N - H bond
They have the same BDE
Depends on temperature
O - H bonds typically have higher BDE (~460 kJ/mol) compared to N - H bonds (~390 kJ/mol) due to stronger orbital overlap and bond polarity. .
How many total electron domains (bonding + lone pairs) surround the nitrogen atom in H2NOH?
2
3
5
4
Nitrogen has three bonds and one lone pair, yielding four electron domains in total. .
In infrared spectroscopy, the O - H stretching frequency in H2NOH is expected around which region?
3200 - 3600 cm?¹
1600 - 1700 cm?¹
4000 - 4500 cm?¹
2000 - 2200 cm?¹
Hydroxyl O - H stretching vibrations typically appear broad around 3200 - 3600 cm?¹ in IR spectra due to hydrogen bonding. .
Upon protonation of H2NOH in acidic solution, which atom is preferentially protonated?
Neither
Both equally
Oxygen
Nitrogen
Protonation occurs primarily at the nitrogen atom, forming NH3OH?, because the nitrogen lone pair is more basic than the oxygen lone pairs. .
What is the molecular point group of H2NOH in its equilibrium geometry?
C1
C2v
C2
Cs
H2NOH has no symmetry planes or rotational axes beyond identity, so it belongs to the C1 point group. .
In proton NMR spectroscopy, the chemical shift of the O - H proton in H2NOH typically appears in which range?
0 - 2 ppm
4 - 6 ppm
2 - 3 ppm
8 - 10 ppm
Alcohol and hydroxyl protons usually resonate between 4 - 6 ppm, though exact shifts depend on hydrogen bonding and solvent. .
0
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Study Outcomes

  1. Analyze electron distribution in H2NOH -

    Interpret how bonding and lone pair electrons are arranged in the Lewis structure of H2NOH to reveal atomic interactions.

  2. Construct accurate Lewis structures for H2NOH -

    Apply valence electron counting and the octet rule to draw a correct Lewis structure of H2NOH with proper formal charges.

  3. Determine formal charges and bond orders -

    Calculate formal charges on each atom in H2NOH and evaluate bond orders to assess molecular stability.

  4. Predict molecular geometry using VSEPR theory -

    Use the VSEPR model to forecast the three-dimensional shape and bond angles of the H2NOH molecule.

  5. Apply structure principles to related compounds -

    Extend your understanding of Lewis structure rules from H2NOH to draw advanced molecules such as XeBr4 correctly.

  6. Evaluate quiz performance for exam readiness -

    Analyze your quiz results to identify strengths and areas for review in preparation for chemistry exams.

Cheat Sheet

  1. Valence Electron Count & Skeleton -

    When constructing the lewis structure of h2noh, start by summing valence electrons: N has 5, O has 6, and each H contributes 1, giving 14 total. Sketch a skeleton with N central bonded to two H atoms and the OH group, ensuring that all atoms can accommodate an octet (H needs only 2 electrons). (Source: University of California, Chemistry Essentials)

  2. Formal Charge Optimization -

    Calculate formal charges using FC = valence electrons - nonbonding electrons - ½ bonding electrons to ensure the most stable arrangement. In NH2OH, both N and O should end up with zero or minimal formal charges for maximum stability. (Source: Royal Society of Chemistry)

  3. Hybridization & Molecular Geometry -

    Assign sp3 hybridization to both N and O based on four electron domains (including lone pairs), predicting a roughly tetrahedral arrangement around each atom. Expect H - N - H bond angles around 107° and H - O - N angle near 104°, reflecting lone”pair repulsion. (Source: American Chemical Society)

  4. Polarity & Hydrogen Bonding -

    With N - H and O - H bonds, NH2OH is polar and can form intra- and intermolecular hydrogen bonds, enhancing solubility. Remember the mnemonic "δ+ on H to δ− on O/N" to predict dipole directions in advanced chemistry test questions. (Source: Journal of Chemical Education)

  5. VSEPR Comparison: NH2OH vs. XeBr4 -

    Contrast the lewis structure h2noh with XeBr4: NH2OH has sp3 domains leading to bent geometry, while XeBr4 has an AX4E2 pattern yielding square planar shape. Use this comparison in your chemistry exam quiz to reinforce VSEPR theory and recognition of lone pairs. (Source: Khan Academy)

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