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Chemistry > Chapter 6-7: Ionic and Metallic Bonding > Flashcards

Chapter 6-7: Ionic and Metallic Bonding Flashcards

1
Q

What is the formula for lead(II) nitrate?

A

Pb(NO3)2

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1
Q

What is the name of the compound Sr(NO2)2?

A

Strontium nitrite

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2
Q

A regular, repeating, three dimensional array of atoms, molecules or ions that minimizes energy.

A

Crystal

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2
Q

Using electron dot structures, predict the formula for rubidium phosphide.

A

Rb3P

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2
Q

What is the formula for nickel(III) sulfide?

A

Ni2S3

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3
Q

A charged group of covalently bonded atoms.

A

A polyatomic ion

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4
Q

Which of the following would you expect to have a higher melting point? Why?

KCl or CaCl2

A

CaCl2 should have the higher melting point. Calcium is a smaller ion than potassium, causing the charges to be closer together, and the lattice energy to be stronger. Additionally, the calcium ion has a +2 charge, but the potassium ion has only a +1 charge. Lattice energies (and thus melting points) are higher for ions having higher magnitude charges.

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4
Q

A rule that states that atoms form compounds in order to achieve 8 valence electrons (a noble gas electron configuration).

A

The octet rule

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4
Q

The collection of a metal’s delocalized valence electrons that move freely throughout the metal, shared by all of the metal’s cation cores.

A

Electron sea

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4
Q

What is the name of the compound MgCl2?

A

Magnesium chloride

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5
Q

A compound composed of only 2 different elements; a monatomic cation and a monatomic anion. Their names always end in -ide.

A

Binary ionic compound

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6
Q

How many total electrons are there in the phosphide ion, P-3?

A

18

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8
Q

A chemical bond that results from the electrical attraction between cations and anions.

A

Ionic bond

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9
Q

What is the name of the compound KOH?

A

Potassium hydroxide

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10
Q

The chemical bonding that results from the attraction between metal cation cores and the surrounding sea of electrons.

A

Metallic bonding

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10
Q

The amount of energy as heat required to vaporize a metal. It is a measure of the strength of the bonds that hold the metal together.

A

Enthalpy of vaporization

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12
Q

Which of the following would you expect to have a higher melting point? Why?

KF or KBr

A

KF should have a higher melting point than KBr. Fluoride and bromide ions have the same charge (-1), but the ionic radius of fluoride is much smaller than that of bromide. This results in a higher lattice energy since the positive and negative charges are closer together.

13
Q

A polyatomic ion containing oxygen.

A

Oxyanion (or oxoanion)

15
Q

A compound composed ot positive and negative ions (cations and anions) that are combined so that the numbers of positive and negative charges are equal.

A

An ionic compound

16
Q

The ability of a substance to be pulled into a wire.

A

Ductility

17
Q

What is the name of the compound V2S3?

A

Vanadium(III) sulfide

18
Q

Another term for an ionic compound.

A

Salt

20
Q

How many electrons are there in the zinc ion, Zn+2?

A

28 electrons. Metals lose valence electrons when forming ions. A +2 charge means there are two more positively charged protons than negatively charged electrons.

21
Q

Atoms or ions having the same electron configuration like Na+1, Mg+2, O-2, F-1, and Ar are….

A

Isoelectronic

22
Q

What is formula for zirconium oxide?

A

ZrO2

23
Q

A substance that conducts electricty when melted or dissolved in water.

A

Electrolytes

24
Q

The ability of a substance to be hammered into thin sheets.

A

Malleability

25
Q

Adjective that describes the mobile valence electrons of a metal.

A

Delocalized

26
Q

What is the formula for ammonium phosphate?

A

(NH4)3PO4

28
Q

The naming system that uses Roman numerals to indicate the charge of the ions of elements which can have multiple ions. For example: iron(III), copper(I), lead(IV).

A

Stock system

29
Q

Using electron dot structures, predict the formula for scandium flouride.

A

ScF3

30
Q

An ion that results from either the gain or loss of one or more electrons by a single atom.

A

Monatomic ion

31
Q

Which substance would you expect to shatter when struck with a hammer? Why?

Aluminum or aluminum oxide

A

Aluminum oxide would shatter. It is an ionic compound, It has a fixed crystal lattice. Striking it with a hammer would cause a shift in the ions that would put like-charged ions beside each other. The resulting repulsion would cause it to shatter. This is why ionic compounds are brittle. Aluminum metal simply dents when struck as the cation cores and sea of electrons simply shift in response to the impact.

33
Q

The energy released when one mole of ionic crystalline compound is formed from gaseous ions.

or

The change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase

A

Lattice energy

34
Q

The zinc ion’s (Zn+2) electron configuration [Ar]3d10 illustrates what kind of stable electron configuration?

A

A pseudo noble gas electron configuration.

35
Q

What is the formula for sodium sulfate?

A

Na2SO4

37
Q

The lowest whole number ratio of cations to anions in an ionic compound.

or

The simplest collection of atoms from which an ionic compound’s formual can be written.

A

Formula Unit

38
Q

What is the name of the compound SnO2?

A

Tin(IV) oxide

39
Q

The formula for the iodate ion is IO3-1. What is the expected formula for the iodite ion?

A

IO2-1. Changing the suffix of a polyatomic ion from -ate to -ite involves removing an oxygen while keeping the charge the same.

40
Q

An ion that is formed as a result of a single atom either gaining or losing electrons?

A

A monatomic ion

41
Q

All monatomic ions have this ending.

A

-ide (like fluoride, telluride, oxide, bromide, etc…)

Chemistry (13 decks)

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