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48 Cards in this Set
- Front
- Back
What is a chemical bond?
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Mutual electrical attraction between the nuclei & valence electrons of different atoms.
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Explain the difference between ionic and covalent bonds in terms of electrons.
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Covalent bonds share electrons --- In ionic bonds, electrons are attracted to the nucleus of another.
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How does a polar covalent bond differ from a non-polar covalent bond?
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Polar--> unequal sharing of electrons
Non-Polar---> equal electron sharing |
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Define "molecule"
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Neutral group of covalently bonded atoms.
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What is a molecular formula?
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Type and number of atoms needed to make a molecule.
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Longer bonds tend to be ___________ than shorter bonds.
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Weaker
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How many valence electrons do atoms seek to achieve?
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8
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Define an ionic compound.
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Postitive and negative ions that have a net charge of zero.
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What is an anion?
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A negative ion
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What is a cation?
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A positive ion
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What is the difference between a covalently bonded "molecule" and an ionicly bonded "crystal" in terms of atoms?
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Ionic-lowest ratio
Covalent- exact # |
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How do covalent and ionic bonded substances differ in properties?
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Covalent-->low melting point, don't conduct electricity, don't dissolve in water
Ionic--->high melting point, conduct electricity, dissolve in water |
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Ammonia is polar because its shape is _____________.
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Pyramidal
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What are the 3 types of bond?
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Covalent, Ionic, & Metallic.
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What is the difference between polar and non-polar bonding?
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Polar---> unequal sharing of electrons
Non-Polar---> equal sharing |
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If the difference in electronegativity is between two atoms is less that 1.0 it is _____(1)______, if the difference in electronegativities is greater than 1.7 it is _____(2)______ , & if the difference is between 1.0 & 1.7 it is ________(3)_________.
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1. Non-Polar Covalent
2. Ionic 3. Polar Covalent |
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When electrons are shared between atoms, are the electrons in a higher or lower energy state than when they are in separate atoms?
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Lower
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What is a molecule?
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Covalently bonded atoms.
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A _________________ shows the number & type of atoms in a molecule.
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Molecular Formula
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The attraction between the _______(1)________ of one atom and the ________(2)_________ of another atom cause the potential energy to be at its lowest and a bond to form.
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1. Nucleus
2. Electrons |
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Define "bond length".
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The average distance between 2 atoms.
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Define "bond energy". What compounds are more stable: ones with high bond energy or ones with low bond energy.
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Bond energy is energy required to break a bond. Compounds with high bond energy are more stable.
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As bond length increases the bond energy ____________.
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Weakens
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Shorter bonds are __________ than longer bonds.
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Stronger
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State the octet rule.
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All atoms want 8 valence electrons.
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What is an unshared pair of electrons?
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Unbonded pairs of electrons on the center atom.
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Write the formula unit for the ionic compound formed by Ca2+ and Br-
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CaBr2
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What kind of structure do we find ionic compounds in?
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Crystals
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Explain the metallic bond.
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Attraction between metal atoms and surrounding electrons.
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List some properties of metals.
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Free electrons, ductile, malleable.
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What is an intramolecular force?
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Forces of attraction between molecules.
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What are the three types of intramolecular forces? List them in order from strongest to weakest.
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Dipole-Dipole, Hydrogen, London Dispersion (Van Der Waals)
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Which intramolecular force holds non-polar molecules together?
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London Dispersion (Van Der Waals)
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Word to describe a molecule with an unequal charge distribution.
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Dipole
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Type of bond formed between an active metal and a nonmetal.
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Ionic
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The simultaneous attraction of electrons for the nuclei of two or more atoms is a chemical ______________.
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Bond
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Bonding that is responsible for the relatively high boiling point of water.
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Ionic
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Type of covalent bond found in diatomic molecules,
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Nonpolar
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Particles formed from covalent bonding.
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Molecules
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Compounds with both ionic and covalent bonds contain this type of ion.
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Polyatomic
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Type of bond found in aluminum foil
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Metallic
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The formulas of ionic compounds must be expressed as ____________ formulas.
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Empirical
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The shape of a water molecule.
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Bent
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Type of bond found between nonmetals.
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Covalent
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Type of covalent bonding that is found in the diamond.
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Network
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Type of covalent bond found between atoms of different electronegativity values.
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Polar
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Force of attractive between nonpolar molecules.
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Van Der Waals
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Element with the highest electronegativity value.
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Fluorine
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