Section 2 - Covalent Bonding & Molecular Compounds
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| A neutral group of atoms that are held together by covalent bonds. | Molecule
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| A single molecule of a chemical compound is an individual unit capable of | existing on its own
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| A chemical compound whose simplest units are molecules | molecular compound
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| The composition of a compound is given by its | chemical formula
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| Indicates teh relative number of atoms of each kind in a chemical compound by using atomic symbols and numberical subscripts | chemical formula
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| Shows the types and numbers of atoms combined in a single molecule of a molecular compound | molecular formula
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| A molecule containing only two atoms | Diatomic molecule
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| an example of a diatomic molecule is | Oxygen
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| The relative strength of attraction and repulsion between the charged particles depends on | The distance separating the atoms
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| When the atoms first sense each other, the electron-proton attraction is | stronger than the elecron-electron and proton-proton repulsions.
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| The bottom of the valley in the curve of an atom energy graph represents | The balance between attraction and repulsion in a stable covalent bond.
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| The distance between two bonded atoms at their miniumum potential energy, that is, the average distance between two bonded atoms is | bond length
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| What is the bond length of a hydrogen-hydrogen bond | 75 pm
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| The amount of energy released equals the difference between the potential energy at zero level (separated atoms) and what | that at the bottom to the valley (bonded atoms).
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| The energy required to break a chemical bond and form neutral isolated atoms | Bond energey
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| Scientist usually report bond energies in what | kilojoules per mole (kJ/mol)
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| Kilojoules indicates what | the energy required to break one mole of bonds in isolated molecules
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| What is the Average bond length and Average Bond energy for H - H | Length 75; Energy 436
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| What is the Average bond length and Average Bond energy for F - F | Length 142; Energy 159
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| What is the Average bond length and Average Bond energy for CI - CI | Length 199; Energy 243
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| What is the Average bond length and Average Bond energy for Br - Br | Length 229; Energy 193
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| What is the Average bond length and Average Bond energy for I - I | Length 266; Energy 151
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| What is the Average bond length and Average Bond energy for H - F | Length 92; Energy 569
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| What is the Average bond length and Average Bond energy for H - CI | Length 127; Energy 432
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| What is the Average bond length and Average Bond energy for H - Br | Length 141; Energy 366
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| What is the Average bond length and Average Bond energy for H - I | Length 161; Energy 299
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| What is the Average bond length and Average Bond energy for C - C | Length 154; Energy 346
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| What is the Average bond length and Average Bond energy for C - N | Length 147; Energy 305
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| What is the Average bond length and Average Bond energy for C - O | Length 143; Energy 358
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| What is the Average bond length and Average Bond energy for C - H | Length 109; Energy 418
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| What is the Average bond length and Average Bond energy for C - CI | Length 177; Energy 327
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| What is the Average bond length and Average Bond energy for C - Br | Length 194; Energy 285
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| What is the Average bond length and Average Bond energy for N - N | Length 145; energy 163
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| What is the Average bond length and Average Bond energy for H - H | Length 101; Energy 386
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| What is the Average bond length and Average Bond energy for O - H | Length 96; Energy 459
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| Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electronsin its hightest occupied energy level | Octet rule
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