Chemistry: Atoms First Questions and Correct Answers
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Chemistry: Atoms Firs
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Chemistry: Atoms Firs
Chemistry: Atoms First Questions and Correct
Answers
Chemistry: Atoms First Questions and Correct
Answers
Chemistry: Atoms First Questions and Correct
Answers
Chemistry: Atoms First Questions and Correct
Answers
Chemistry: Atoms First Questions and Correct
Answers
Chemistry: Atoms Fi...
Chemistry: Atoms First Questions and Correct
Answers
Which of the following is a characteristic of ionic solids?
Their ionic bonds are very strong
Ionic solids are poor conductors of electricity
Ionic solids dissolve easily in water
All of the above
✓ ~~~ All of the above
Explanation: The properties of ionic compounds shed some light on the nature of
ionic bonds. Ionic solids exhibit a crystalline structure and tend to be rigid and brittle;
they also tend to have high melting and boiling points, which suggests that ionic
bonds are very strong. Ionic solids are also poor conductors of electricity for the
same reason. Most ionic solids, however, dissolve readily in water.
Ions typically have:
✓ ~~~ properties that are dramatically different from those of the corresponding
neutral atom
Explanation: By definition of an ion, they will always bear an electrical charge, either
positive or negative. Sodium and chlorine are excellent examples of how properties
of individual ions correspond to the properties of the ionic compound. Both sodium
and chlorine are toxic elements individually, but once ionized, are harmless
,components of table salt. Therefore, ions typically exhibit dramatically different
properties from those of the corresponding neutral compound.
Ionic compounds tend to be:
✓ ~~~ Neutral
Explanation: By definition, ionic compounds are composed of both positive cations
and negative anions and bear a neutral overall charge. Therefore, these ions must
come together in a particular ratio so as to result in a neutral substance.
Ionic compounds tend to form between a nonmetal with ________ and a metal with
__________.
✓ ~~~ high electron affinity, low ionization energy
Explanation: Nonmetals tend to have a high electron affinity whereas metals tend to
have low ionization energies. A metal with a low ionization energy can easily lose an
electron. A nonmetal with a high electron affinity can easily gain an electron. Thus if
these elements come into contact, an electron will transfer from the metal to the
nonmetal, forming an ionic compound as a result.
What is the abbreviated electron configuration of Mn2+?
✓ ~~~ [Ar]3d^5
,Explanation: The abbreviated electron configuration of Mn is [Ar]4s23d5. Because
Mn is a d-block transition metal, the electrons of the s subshell are removed before
the (n−1)d electrons. Thus the abbreviated electron configuration for Mn2+ is
[Ar]3d^5.
What is the charge of a yttrium cation?
Only enter the charge of the cation, do NOT enter the element symbol.
✓ ~~~ 3+
Explanation: Yttrium has three valence electrons, and it will typically lose all three to
become the 3+ ion.
What is the charge of a bromine ion?
✓ ~~~ -1
Explanation: The bromide ion is 1 electron away from having a noble gas
configuration so its charge is 1−.
Which of the following anions is most likely to form?
Br2−
S−
Se3−
, Te2−
✓ ~~~ Te^2−
Explanation: Tellurium will tend to gain two electrons to fill its valence shell. Sulfur
and selenium also should become 2−, while bromine should become 1−.
Which of the following statements about nonmetal anions are true?
-Nonmetals tend to form anions by gaining electrons to form a noble gas
configuration.
-Nonmetals do not tend to form anions.
-Anions of nonmetals tend to be isoelectronic with a noble gas.
-Nonmetals tend to form anions by losing electrons to form a noble gas
configuration.
✓ ~~~ Nonmetals tend to form anions by gaining electrons to form a noble gas
configuration.
Anions of nonmetals tend to be isoelectronic with a noble gas.
Explanation: Most monatomic anions form when a neutral nonmetal atom gains
enough electrons to completely fill its outer s and p orbitals (valence orbitals),
thereby reaching the electron configuration of the next noble gas. Anions that have
the same number of electrons as the next noble gas makes the anion isoelectronic
with the noble gas.
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