Questions from Organic Chemistry
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Questions from Organic Chemistry - Leaderboard
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42 questions
| 🇬🇧 | 🇬🇧 |
| Atoms with the same number of protons but different numbers of neutrons are called __________. | Isotopes |
| Which of the following elements does this electronic configuration represent? 1s2 2s2 2p5 F C N Al O | F |
| Which of the following is the electronic configuration of the element Fe? | 1s2 2s2 2p6 3s2 3p6 4s2 3d6 |
| Which of the following statements correctly describes the third electron shell that surrounds the nucleus of an atom? | The maximum number of electrons that can occupy the third shell is 18. |
| Which of the following describes a hydride ion? | A negatively charged hydrogen ion containing a pair of electrons |
| Using the symbol δ+ and δ-, indicate the direction of the polarity in the indicated bond. | Down below δ- δ+ .. CH3O--H .. |
| Covalent bonds may be polar or nonpolar. What property of the atoms forming a given bond determines this? | Electronegativity |
| The compound methylamine, H3C-NH2, contains a C-N bond. In this bond, which of the following best describes the charge on the nitrogen atom? | Slightly negative |
| Which of the following structures, including formal charges, is correct for diazomethane, H2CN2? | Here on first N + Second N - |
| What are the formal charges on nitrogen and the starred oxygen atom in the following molecule? | N= +1, O = 0 |
| Draw condensed structures for the four compounds with formula C3H9N. | CH3CH2CH2NH2 CH3CH2NHCH3 (CH3)2CHNH2 (CH3)3N |
| Both sigma (σ) and pi (π) bonds can be formed by overlapping p orbitals. Describe the difference. | Sigma bonds are formed from the overlap of atomic orbitals along a circular axis of symmetrical nature, i.e., head-on overlap. All single bonds are sigma bonds. Pi bonds are formed from the overlap of atomic orbitals along a non-symmetrical (parallel) axis, i.e., side-to-side overlap. Double and triple bonds are pi bonds. |
| What orbitals are used to form the covalent bonds in butane (CH3CH2CH2CH3)? | The carbon-carbon σ bonds are formed by the overlap of two carbon sp3 hybrid atomic orbitals. The carbon-hydrogen σ bonds are formed by the overlap of a carbon sp3 hybrid atomic orbital and a hydrogen s orbital. |
| Which of the following is a correct formula for a compound? | CH3CH(CH3)CH2CH3 |
| Which of the following describes a triple bond? | One sigma bond and two pi bonds |
| What is the predicted shape, bond angle, and hybridization for +CH3? | Trigonal planar, 120°, sp2 |
| Explain why the water molecule has a bent shape and a bond angle less than 109.5°. | The electron replusion between the two lone pairs of electrons on the oxygen of water causes the O-H bonds to squeeze close together. |
| The carbon- carbon double bond in ethene is __________ and __________ than the carbon-carbon triple bond in ethyne. | Weaker; longer |
| Why is the C H bond in ethene (H2CCH2) shorter and stronger than the C H bond in ethane(H3C-CH3)? | The length and strength of a C H bond depends on the hybridization of the carbon atom. The more s character in the hybrid orbital used by carbon to form the bond, the shorter and stronger the bond. This is because an s orbital is closer to the nucleus than is a p orbital. Ethene uses carbon sp2 hybridized orbitals (1/3 s character) to make its carbon-hydrogen bonds while ethane uses carbon sp3 (1/4 s character) orbitals. |