Chapter 6 Sect. 1-2 Review – Flashcards
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Ionic bonds form as a result of the electrostatic attraction between
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ions
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A single covalent bond involves the sharing of
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two electrons
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The measure of an atom's ability to attract electrons is its
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electronegativity
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Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be
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nonpolar-covalent compounds
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What is the apparent charge on the chlorine atom in the molecule HCl?
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8-
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Atoms seldom exist as independent particles in nature because
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atoms are more stable when they combine with other atoms
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When an atom completely gives up its valence electrons to another atom, they form a bond that is considered to be
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purely ionic
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You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the
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difference in the atoms' electronegativities
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A chemical bond between atoms results from the attraction between the valence electrons and ____ of different atoms
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nuclei
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A covalent bond consists of
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a shared electron pair
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If two covalently bonded atoms are identical, the bond is identified as
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nonpolar covalent
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A covalent bond in which there is an unequal attraction for the shared electrons is
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polar
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Atoms with a strong attraction for electrons they share with another atom exhibit
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high electronegativity
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Bonds that possess between 5% and 50% ionic character are considered to be
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polar covalent
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The greater the electronegativity difference between two atoms bonded together, the greater the bond's percentage of
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ionic character
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The electrons involved in the formation of a chemical bond are called
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valence electrons
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A chemical bond that results from the electrostatic attraction between positive and negative ions is called an
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ionic bond
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If electrons involved in bonding spend most of the time closer to one atom rather than the other, the bond is
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polar covalent
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If a bond's character is more than 50% ionic, then the bond is called an
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ionic bond
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A bond's character is more than 50% ionic if the electronegativity difference between the two atoms is greater than
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1.7
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Write the formula for an example of each of the following compounds:
a. nonpolar covalent compound
b. polar covalent compound
c. ionic compound
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a. H2 (two is the bottom number, like in H2O)
b. HCl
c. NaCl
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Describe how a covalent bond holds two atoms together.
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A pair of electrons is attracted to both nuclei of the two atoms bonded together.
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What property of the two atoms in a covalent bond determines whether or not the bond will be polar?
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Electronegativity difference
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How can electronegativity be used to distinguish between an ionic bond and a covalent bond?
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The difference between the electronegativity of the two atoms in a bond will determine whether the bond is ionic or covalent. If the difference in electronegativity is greater than 1.7, it is ionic.
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Describe the electron distribution in a polar-covalent bond and its effect on the partial charges of the compound.
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The density is greater around the more electronegative atom so the electrons go to the more negative atom.
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If two covalently bonded atoms move closer than a distance of the bond length, the potential energy of the atoms
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increases
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The electrons involved in the formation of a covalent bond are
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valence electrons
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Bond energy is the energy
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required to break a chemical bond and form separate, neutral atoms
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Bond length between two bonded atoms is
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the separation at which their potential energy is minimum
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The Lewis structure of which of the following compounds does not follow the octet rule?
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BF3
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In a double covalent bond,
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two atoms share two pairs of electrons
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Which of the following is not a resonance structure of SO3?
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D
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How many double bonds are in the Lewis structure for hydrogen fluoride, HF?
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none
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To draw a Lewis structure, it is not necessary to know
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the length of the bonds
