or Create Online Test

Reveal Answers: During the Quiz (Practice Mode) End of Quiz (Exam Mode) Number of questions: All 123456789101112131415161718192021222324252627282930313233343536373839404142434445464748

Changes are done, please start the quiz.

1.	A chemical bond is the attraction between a positive nucleus and negative electrons, or positive and negative ions. True or False?

A.

True

B.

False

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.

cations

B.

anions

C.

electrons

D.

nuclei

E.

photons

6.	Noble gases have:

A.	low ionization energy and high electron affinity

B.	high ionization energy and low electron affinity

C.	the same amount of ionization energy as electron affinity

7.	The number of valence electrons can be directly related to the difference in reactivity.

A.

True

B.

False

8.	An Ionic compound with 2 elements, containing one metal cation and one nonmetal anion, is known as:

A.	Monoatomic Ionic Compound

B.	Polyatomic Ionic Compound

C.	Binary Ionic Compound

D.	Binary Element

9.	Metals are ______, while nonmetals are _______.

A.	anion, cation

B.	brittle, malleable

C.	gypsies, thieves

D.	cation, anion

10.	The electrostatic force that holds oppositely charged particles together in an ionic compound is known as:

A.	Electromagnetitivity

B.

A Cation

C.	Electron Affinity

D.	Ionic Bond

E.	Chemical-Covalent Bond

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.	The ionic pyramid of charges

B.	Crystal Lattice

C.	Electron Affinity Model

D.	Sea of Electrons Model

12.	What does conductivity of an ionic compound depend upon?

A.	The cardinal charge of the cation

B.	The cardinal charge of the anion

C.	Lattice Energy and how it affects the ionic compound

D.	Whether the ionic compound is a monoatomic compound or a binary compound

E.	The free-moving ability of electrons

13.	Ionic crystals typically have _____ melting and boiling points because of strong, attracted forces. Similarly, ionic crystals are ______ when solid.

A.	high, nonmalleable

B.	low, nonmalleable

C.	high, malleable

D.	low, nonmalleable

14.	An Ionic compound whose acqueous solution conducts an electric current is known as:

A.	Delocalized Ionic Compound

B.	Polyatomic Ionic Compound

C.	Binary Ionic Compond

D.	Electrolyte

E.	Crystal Lattice

15.	The energy required to separate one mole of the ions of an ionic compound is:

A.	Electron Affinity

B.	Lattice Energy

C.	Ionization Energy

D.	Electromagnetitivity

E.	Monoatonomy

16.	The _____ the lattice energy, the stronger the force of the attraction is.

A.

greater

B.

lesser

17.	The smaller the ions are, the ________ the lattice energy is because of interionic attraction due to there being a _____ distance between charges

A.	greater, greater

B.	greater, smaller

C.	smaller, greater

D.	smaller, smaller

18.	A formula unit (chemical formula for an ionic compound) is always ____ in charge.

A.

positive

B.

negative

C.

neutral

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.	monoatomic

B.	polyatomic

C.

binary

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.	lattice energy

B.	formula unit

C.	electrostatic attraction

D.	oxidation number

21.	An Ion made of more than 1 atom is:

A.	Monoatomic

B.

Binary

C.	Polyatomic

22.	A(n) _____ is a polyatomic ionic compound composed of an element, usually a nometal, bonded to one or more oxygen atoms.

A.	oxidation state

B.

oxyanion

C.

oxion

D.

oxanion

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.	"Ate" will always have a superscript that is 1 greater than "ite".

B.	"Ite" will always have a superscript that is 1 greater than "ate."

C.	"Ite" will always have a superscript that is 3 times as that of "ate."

24.	___________ Ionic compounds always end in "ide."

A.	Monoatomic

B.

Binary

C.	Polyatomic

25.	What is the name of CsBr?

A.	Cesium Bromate

B.	Cesium Bromite

C.	Celium Bromide

D.	Cesium Bromide

E.	Celium Bromite

26.	Ionic compounds that are liquid conduct electricity because:

A.	The difference of the atomic mass between an ion and an atom

B.	(of) Delocalized electrons

C.	They are Interstitial alloys

D.	They are Substitutional alloys

27.	The attraction of a metallic cation for delocalized electrons is known as a(n):

A.	Ionic Bond

B.	Chemical Bond

C.	Physical Bond

D.	Covalent Bond

E.	Metallic Bond

28.	What is the difference between a substitutional and an interstitial alloy?

A.	Substitutional alloys consist of small holes in a metallic crystal, while interstitial intersect atoms in substitutional alloys.

B.	Substitutional alloys are replaced by other metals of opposite atomic size, while interstitial alloys intersect the electrons of a substitutional alloy (thus preventing from combining).

C.	Substitutional alloys are replaced by other metals of similar atomic size, while interstitial alloys have small hols in a metallic crystal that are filled with smaller atoms.

D.	Substitutional alloys substitute interstitial alloys when the interstitial alloy is not durable enough for the product being manufactured.

29.	Nonmetals form a stable outer electron configuration by losing electrons and becoming anions.

A.

True

B.

False

30.	A Cl - ion is an example of a cation.

A.

True

B.

False

31.	A sodium atom tends to lose one electron when it reacts.

A.

True

B.

False

32.	Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge.

A.

True

B.

False

33.	A positively charged ion is called an anion.

A.

True

B.

False

34.	Elements tend to react so that they can acquire the electron struture of a noble gas.

A.

True

B.

False

35.	The ending "ide" is used to designate an anion.

A.

True

B.

False

36.	H+ would be called a Hydrogen ion and not hydride.

A.

True

B.

False

37.	N+ would be called nitride and not a nitrogen ion.

A.

True

B.

False

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.

True

B.

False

39.	Salts are examples of ionic compounds.

A.

True

B.

False

40.	The crystal lattice of ionic compounds affect their melting and boiling points.

A.

True

B.

False

41.	The lattice energy is the energy required to separate the ions of an ionic compound.

A.

True

B.

False

42.	The energy of an ionic compound is higher than that of the separate elements that formed it.

A.

True

B.

False

43.	Large ions tend to produce a more negative value for lattice energy than smaller ions do.

A.

True

B.

False

44.	Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.

A.

True

B.

False

45.	Steel is an example of an ____ alloy.

A.	substitutional

B.	interstitial

C.	monoatomic

46.	Why do we "criss-cross"?

A.	To get a more negative charge.

B.	To get a more stable charge.

C.	To get a more positive charge.

47.	Higher oxidation state = ____ Lattice Energy.

A.

Lower

B.

Higher

48.	Ionic compounds are conductive only when a liquid/acqueous.

A.

True

B.

False