Memorize Chemical Bonding: 85 Flashcards on Ionic, Covalent, Metallic and Hydrogen Bonds
Memorize chemical bonding with 85 real flashcards: ionic, covalent and metallic bonds, sigma and pi bonds, electronegativity, VSEPR, MO theory and bond energies.
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Chemical Bonding (GK6598) has 85 cards, and most of them come from one long encyclopedia article on the chemical bond. That shows in the order: types of bonds first (1-22), then a history detour (23-33: Lavoisier, Abegg, Nagaoka, Planck, Lewis), then bond orders, ionic crystals, coordinate bonds and intermolecular forces (34-68), the theory debate (69-81), and four hard numbers at the very end (82-85). Rearrange it into a plan and it becomes a solid general-chemistry deck.
Study this deck: Chemical Bonding
1 / 10Chemical bond
Tap the card for the answer · swipe right if you knew it, left if not
A sample of the real cards
| Front | Back |
|---|---|
| Three types of strong or primary bonds | Covalent, ionic and metallic bonds |
| In an ionic bond, what happens to the bonding electron? | It is transferred from one atom to another, not shared |
| Why are ionic substances brittle? | Forces between ions are short-range and do not bridge cracks |
| Why are metals malleable? | Metallic bonding is collective, with no particularly oriented bonds |
| Triple bond | Three shared electron pairs: one sigma and two pi bonds |
| Example of a coordinate covalent bond | F₃B←NH₃, a B-N bond from a nitrogen lone pair |
| Hydrogen bonds responsible for | The high boiling points of water and ammonia vs their heavier analogues |
| N≡N triple bond energy | 945 kJ/mol (bond length 110 pm) |
Vocabulary you'll own
Covalent, polar covalent and non-polar covalent bonds (CH₄), ionic bonds and ionic crystals (NaCl, NaCN), metallic bonding and the electron sea, electronegativity and the 1.7 rule of thumb, single, double and triple bonds, sigma and pi bonds, coordinate (dative) bonds, Lewis acids and bases, transition metal complexes (Ag(NH₃)₂⁺), the octet rule, Lewis structures, VSEPR, valence bond theory, hybridization and resonance, molecular orbital theory, density functional theory, oxidation number, formal charge, intermolecular forces, Van der Waals, Keesom and London dispersion forces, hydrogen and halogen bonds, X-ray diffraction, bond length and bond energy.
Study it in this order
- Bond types and properties (1-22, 34-60): learn each bond with the property it explains — brittle salts, malleable metals, shiny conductors, high-melting diamond and quartz.
- Intermolecular forces (61-68): keep them separate from the strong bonds; they explain melting and boiling points.
- Theories (6-10, 69-81): VB = localized pairs, MO = delocalized orbitals; both are right.
- History (23-33) last, or suspend it if your exam does not ask for it.
Two tips specific to this deck
Turn the last four cards into a trend. H-H (74 pm, 436 kJ/mol), C=C (134 pm, 614), C≡C (120 pm, 839) and N≡N (110 pm, 945) are the only numbers in the deck. Add the missing C-C single bond (154 pm, about 347 kJ/mol) and you get the rule exams test: higher bond order → shorter and stronger bond, though a double bond is not twice as strong as a single.
Fill the gaps the deck names but never teaches. VSEPR is defined (card 8) but no shape appears — write cards for linear, trigonal planar, tetrahedral (CH₄, 109.5°), trigonal pyramidal (NH₃) and bent (H₂O). Hybridization is mentioned (card 74) with no sp, sp² or sp³ example. And the 1.7 electronegativity cut-off (cards 39-40) is a convention, not a law: add the other common boundary, below about 0.4 = non-polar covalent, so polar covalent gets its own range.
Electronegativity values come from the periodic table, so review it alongside all 118 elements; sigma and pi bonds return in organic chemistry structure.
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