Chapter 6 Test
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| How does a covalent bond form between two atoms? | shares atams
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| How does a covelent bond differ from an ionic bond? | ionic steals. covalent shares.
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| What is a molecular bond? | space that shares electrons move within
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| Bond ______ is defined as the average distance between two bonded atoms at their minimum potential energy. | length
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| Bond ______ is defined as the energy required to break the chemical bond between two atoms and separate them. | energy
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| The tendency of an atom to attract bonding electrons to itself when it bonds with another atom is called its _________. | electronegitivity
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| A ________ bond is an attraction between two atoms in which bonding electrons are localized on the more electronegative atom. | polar covalent
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| A ________ bond is an attraction between two atoms in which bonding electrons are shared equally between the atoms. | non-polar covalent
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| A ________ molecule is one that has a partial positive charge at one end and a partial negative at the opposite end. | dipole
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| In general, if the difference in electronegativity between two atoms is between 0 and 0.5, that bond formed is ________. | non-polar covalent
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| If the elecronegitivity difference between two atoms is between 0.5 and 2.1, the bond formed is _______. | polar covalent
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| If the electronegativity difference between two atoms is greater than 2.1, the bond formed is _______. | ionic
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| Name the bond (ionic/covalent) in NaF | ionic
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| Name the bond (ionic/covalent) in polyethylene (carbon/hydrogen) | covalent
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| Name the bond (ionic/covalent) between carbon and sulfur | covalent
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| Name the bond (ionic/covalent) between carbon and fluorine | covelent
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| Name the bond (ionic/covalent) between phosphorus and oxygen | covelent
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| An electron in the outermost energy level of an atom that can participate in bonding is called a ________ electron. | valence
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| A structure in which atomic symbols represent nuclei and inner-shell electrons and in which dots are used to represent valence electrons is called a ______ electron. | Lewis
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| A covalent bond in which two atoms share two pairs of electrons is called a _________ bond. | double
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| A covalent bond in which two atoms share three pairs of electrons is called a _______ bond. | triple
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| A covalent bond in which two atoms share one pair of electrons is a ________ bond. | single
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| A non-bonding pair of electrons in the valence shell of an atom is called a _______ pair. | unshared
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| PbCl^2 | Lead (ii) chloride
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| KCl | Potassium chloride
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| LiO^2 | Lithium peroxide
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| PBr^3 | Phosphorus triboride
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| SF^4 | Sodium tetrafloride
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| N^2O^5 | Dinitrogen pentaoxide
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| Nitrogen monoxide | NO
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| Carbon dioxide | CO^2
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| Carbon tetrachloride | CCl^4
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| Carbon disulfide | CS^2
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| What does VSEPR theory predict? | predict shape
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| What is the VSEPR theory? | VALENCE SHELL ELECTRON PAIR REPULSION
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| How does one unbonded pair of electrons (a lone pair) affect the shape of a molecule? | assemetrical
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| How do multiple unbonded pairs of electrons affect the shape of a molecule? | repeal each other (bent)
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| What evidence is there to support the idea that opposite polar ends of molecules attract each other? | it changes properties (magnet w/ water)
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| How do polarity and shape of molecules relate to the properties of a substance? | boiling points differ
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