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Chapter 7 Chem: Practice Test

48 Questions  I  By Konlee
Chapter 7 Chem: Practice Test
Yay, this practice test will determine if you're ready to take the real thing. Questions are taken right out of the book/packet and review lotsa vocab.

  
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Question Excerpt

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1.  A chemical bond is the attraction between a positive nucleus and negative electrons, or positive and negative ions. True or False?
A.
B.
2.  A _____  ______ is a force that holds two atoms together.
3.  Atoms that acquired a positive or negative charge are called ____.
4.  The energy required to lose an electron is known as __________ ______.
5.  Electron affinity is the amount of attraction an atom has for _______.
A.
B.
C.
D.
E.
6.  Noble gases have:
A.
B.
C.
7.  The number of valence electrons can be directly related to the difference in reactivity.
A.
B.
8.  An Ionic compound with 2 elements, containing one metal cation and one nonmetal anion, is known as:
A.
B.
C.
D.
9.  Metals are ______, while nonmetals are _______.
A.
B.
C.
D.
10.  The electrostatic force that holds oppositely charged particles together in an ionic compound is known as:
A.
B.
C.
D.
E.
11.  Large numbers of positive ions and negative ions exist together in a ratio determined by the number of electrons transferred from the metal atom to the nonmetal atom. These ions are packed in a regular, repeating pattern that balances the forces of attraction and repulsion between the ions. This regular, repeated pattern in a 3-dimensional geometric arrangement is known as:
A.
B.
C.
D.
12.  What does conductivity of an ionic compound depend upon?
A.
B.
C.
D.
E.
13.  Ionic crystals typically have _____ melting and boiling points because of strong, attracted forces. Similarly, ionic crystals are ______ when solid.
A.
B.
C.
D.
14.  An Ionic compound whose acqueous solution conducts an electric current is known as:
A.
B.
C.
D.
E.
15.  The energy required to separate one mole of the ions of an ionic compound is:
A.
B.
C.
D.
E.
16.  The _____ the lattice energy, the stronger the force of the attraction is.
A.
B.
17.  The smaller the ions are, the ________ the lattice energy is because of interionic attraction due to there being a _____ distance between charges
A.
B.
C.
D.
18.  A formula unit (chemical formula for an ionic compound) is always ____ in charge.
A.
B.
C.
19.  Note: the characters after the " ^ " are meant to be held up in superscript.Is the following a monoatomic, polyatomic, or binary ion? Mg ^ 2+ 
A.
B.
C.
20.  The charge of a monoatomic ion is equal to the number of electrons transferred from the atom to the ion. This is called:
A.
B.
C.
D.
21.  An Ion made of more than 1 atom is:
A.
B.
C.
22.  A(n) _____ is a polyatomic ionic compound composed of an element, usually a nometal, bonded to one or more oxygen atoms.
A.
B.
C.
D.
23.  When naming oxyanions, it is likely that you will use "ate" or "ite", like "Nitrate" and "Nitrite."Which of the following statements, knowing this, is true?
A.
B.
C.
24.  ___________ Ionic compounds always end in "ide."
A.
B.
C.
25.  What is the name of CsBr?
A.
B.
C.
D.
E.
26.  Ionic compounds that are liquid conduct electricity because:
A.
B.
C.
D.
27.  The attraction of a metallic cation for delocalized electrons is known as a(n):
A.
B.
C.
D.
E.
28.  What is the difference between a substitutional and an interstitial alloy?
A.
B.
C.
D.
29.  Nonmetals form a stable outer electron configuration by losing electrons and becoming anions.
A.
B.
30.  A Cl - ion is an example of a cation.
A.
B.
31.  A sodium atom tends to lose one electron when it reacts.
A.
B.
32.  Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge.
A.
B.
33.  A positively charged ion is called an anion.
A.
B.
34.  Elements tend to react so that they can acquire the electron struture of a noble gas.
A.
B.
35.  The ending "ide" is used to designate an anion.
A.
B.
36.  H+ would be called a Hydrogen ion and not hydride.
A.
B.
37.  N+ would be called nitride and not a nitrogen ion.
A.
B.
38.  When naming ions, a positive ion would be called [insert element here] anion, while a negative ion would be given the suffix "ide."
A.
B.
39.  Salts are examples of ionic compounds.
A.
B.
40.  The crystal lattice of ionic compounds affect their melting and boiling points.
A.
B.
41.  The lattice energy is the energy required to separate the ions of an ionic compound.
A.
B.
42.  The energy of an ionic compound is higher than that of the separate elements that formed it.
A.
B.
43.  Large ions tend to produce a more negative value for lattice energy than smaller ions do.
A.
B.
44.  Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.
A.
B.
45.  Steel is an example of an ____ alloy.
A.
B.
C.
46.  Why do we "criss-cross"?
A.
B.
C.
47.  Higher oxidation state = ____ Lattice Energy.
A.
B.
48.  Ionic compounds are conductive only when a liquid/acqueous.
A.
B.
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