CHEMISTRY - BROWN 13E CH.22 - CHEMISTRY OF THE...

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CHEMISTRY - BROWN 13E

CH.22 - CHEMISTRY OF THE NONMETALS

CONCEPT: HYDROGEN CHEMISTRY The hydrogen atom represents the simplest of the elements of the Periodic Table and consists of ____ proton and ____

electron.

Elemental hydrogen will react with elements to form either ionic or covalent hydrides.

• When reacting with Group 1A elements, the heavy Group 2A elements: ______ , ______ or ______ and other reactive metals.

• These compounds tend to be white, crystalline solids.

2 K (s) + H2 (g)

Ba (s) + H2 (g)

• The hydride ion can also act as a ____________ agent and donate its electrons or as a ___________ base.

SiBr3 (l) + NaH (g)

HCl (aq) + NaH (g)

• When reacting with nonmetals.

3 H2 (g) + N2 (g) 2 NH3 (g) ΔHRxno = − 91.8 kJ

1

H1.01

Ionic Hydrides

Covalent Hydrides



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CONCEPT: ALKALI METALS

Named for the __________ solutions they tend to form during reactions.

• Because of their lower molar masses, larger atomic radii and ns1 electron configuration they tend to be __________ malleable with __________ densities, melting and boiling points.

• Because they are strong reducing agents they naturally occur as _______ cations in nature.

• Almost all the Alkali Metals are water soluble and create highly ____________________ heat of hydration (ΔHhydr ).

• In the process the hydrogen is ______________________ .

2 M (s) + 2 H2O (l) 2 M+ (aq) + 2 OH – (aq) + H2 (g)

• The Alkali Metals react with elemental oxygen to form different types of ________________________ .

Li (s) + O2 (g)

Na (s) + O2 (g)

M (s) + O2 (g)

• The Alkali Metals react with the diatomic halogens to form ________________________ .

2 M (s) + X2 ( X = F, Cl, Br or I )

Reacting with H2O

Reacting with O2

Reacting with Halogens



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CONCEPT: ALKALINE EARTH METALS Named because their oxides also form basic solutions and because their high temperatures allowed them to remain as a solid (“earth”).

• Their higher temperature is the result of an additional valence electron: ns2 electron configuration.

• The addition of the valence electron with a minimal change in size results in _____________ metallic

bonding.

• All the Alkaline Earth Metals except for _______ form ionic compounds when bonding to nonmetals.

Physical Properties

Chemical Properties



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CONCEPT: REACTIONS OF ALKALINE EARTH METALS

• Since they can act as strong _____________________ agents they can reduce atmospheric oxygen.

2 M (s) + O2 (g)

• The heavy Group 2A elements: ______ , ______ or ______ reduce water to form elemental hydrogen.

M (s) + 2 H2O (l) M2+ (aq) + 2 OH – (aq) + H2 (g)

• The Alkaline Earth Metals react with the diatomic halogens to form ________________________ .

M (s) + X2 ( X = F, Cl, Br or I )

Reacting with H2O

Reacting with Halogens

Reacting with O2



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• All Alkaline Earth Metal oxides are basic with exception to ___________ .

MO (s) + H2O (l) M2+ (aq) + 2 OH – (aq)

• Carbonate compounds will undergo thermal decomposition to form the oxide.

MO3 (s)

Elemental Oxides

Thermal Decomposition



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CONCEPT: PERIODIC TRENDS OF METALS

_________________________ are similarities that exist between a Period 2 element and another element that is

diagonally lower one level and to the right.

• Both react with elemental nitrogen to form ________________ .

Li (s) + N2 (g)

Mg (s) + N2 (g)

• Both form hydroxides and carbonates that undergo thermal decomposition.

• Both form oxide coatings that prevent reaction with water.

• Both form oxides that are ______________________ .

• Electrical they behave as _____________________.

• In their oxyacid or oxoacid forms they represent ___________________ .

• When combined with a hydride ion they represent _______________________________ .

Lithium & Magnesium

Beryllium & Aluminum

Boron & Silicon

H2SiO3 – Metasilicic Acid H4SiO4 – Silicic AcidH3BO3 – Boric Acid

SiH4 – SilaneBH3 – Borane



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CONCEPT: THE BORON FAMILY Although boron is at the top of Group 3A, it does not represent the general properties of the group because it is sole metalloid.

Physical & Chemical Behavior

*_________________ was formally called _________________.

Physical Properties

- Although the trends are not as uniform throughout Group 3A, we can say generally the boiling points ________________

and ________________ densities when going down the group.

Oxidation States

- The _____ state is the most common form experienced by this group, but as we move down the group the _____ state

becomes more predominant.

- The lower oxidation state of elements tend to be more ___________ than the oxides with the element in a higher oxidation

state.

Element

Bonding

Melting Point (oC)

ΔHFusion (kJ / mol)

B 2180 50.0

Al 660 10.7

Ga 30 5.59

In 157 3.26

Tl 304 4.20

Nh* N/A N/A N/A



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CONCEPT: BORON FAMILY CHEMISTRY The periodic trends of Group 3A are harder to predict as a result of the inclusion of d and f electrons as we move down the group. These irregularities as a result impact the chemical properties of elements.

Chemical Properties

- Boron is the only metalloid in Group 3A and is ________ reactive at room temperature and only forms _______________

bonds.

- Aluminum forms _______________ oxides and when connected to halogens in the gas phase it forms covalent dimers.

- All remaining elements in the group form ionic bonds, however they do contain more covalent character than Group 2A.

Reactions

– Elements within this group react very slowly or not at all with water:

– In the presence of oxygen gas and heat they become oxides:

– When placed next to halogens they undergo oxidation:



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CONCEPT: THE CARBON FAMILY The column containing carbon is unique in that it contains all 3 classifications for elements: _________________, _________________ and _________________.


Ge 945 31.8

Sn 232 7.0

Pb 327 4.77

Fl* N/A N/A N/A


Allotropism

Allotropism is the ability of some elements to exist in different forms while in the same physical state. Carbon for instance has two predominate forms: __________________ and __________________.

Their differences in form can lead to vastly different properties.

__________________ is represented as a soft, black conductor of electricity, while __________________ is considered one of the hardest natural materials in nature that is colorless and is an insulator of electricity.

• A 1980s mass spectroscopic examination of soot discovered another allotropy for carbon known as buckminsterfullerene, or simply __________________.

Element

Bonding

Melting Point (oC)


C 4100 105

Si 1420 50.2



Page 10

CONCEPT: CARBON CHEMISTRY Carbon is one of the most unique elements of the periodic table because of its ability to form covalent bonds with other carbon atoms in a process called ______________________.

• By incorporating other nonmetals it is possible to create diverse organic compounds found in nature.

C

H

H

H

C

H

H

OH

Ethanol

HC C

HCO

H

Cinnamic aldehyde

C

H

H

H

C

O

OH

Acetic Acid

• As you move down the group the atomic radius _____________, which creates longer bonds that are weaker and more open to reactions. As a result none of the other elements form stable chemical chains.

Gaseous Oxides

Inorganic carbon compounds are commonly found with carbonates.

CaCO3 (s) + H2SO4 (aq)

Carbon monoxide, CO, represents another gaseous oxide that is commonly used in industrial production of methanol and methanal. It also plays a disruptive effect in displacing oxygen from hemoglobin.

Halomethanes

Carbon can form strong chemical bonds with halogens to form _____________________________ (CFCs), which have been linked to deterioration of the ozone layer.

C

F

ClClF

C O



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CONCEPT: THE SILICON CHEMISTRY The chemistry of silicon is dominated by the formation of __________________________________ bonds.

• These long repeating chains can be formed naturally into what are called silicates or synthetically created into other structures called silicones.

Silicates

The building block unit for silicates is the ______________________, which is represented by SiO44-.

Si

O

OOO

Orthosilicate ions

Orthosilicate complex

Silicones

Within these structures we have two hydrocarbon groups connect to each silicon atom and those silicon atoms are connected to one another by an oxygen atom.

Si

CH3O

CH3

O Si O Si O Si

CH3

CH3

O

CH3

CH3

CH3

CH3

The ______________________ of the silicones are held by weak intermolecular forces and so experience increased

flexibility, while the ______________________ gives rigidity and stability to the compound.



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CONCEPT: THE NITROGEN FAMILY Due to its position on the periodic table Group 5A shows more diversity than the earlier groups.


The non-predictable behavior of the elements in Group 5A reflects the transition from individual covalent molecules in _____ and _____ to network covalent solids in _____ and _____ to the metallic characteristics of _____ and _____.

Element

Bonding

Melting Point (oC)


N - 210 0.36

P 44.1 0.64

As 816 27.7

Sb 631 19.7

Bi 271 10.9

Mc N/A N/A N/A


Allotropism

Phosphorus (P4) - ________ form is made of individual tetrahedrons, giving them low melting points and high solubility in nonpolar solvents. ________ Reactivity. - ________ form exists in chains; making them have higher melting points, lower solubility in nonpolar solvents. ________

Reactivity.



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CONCEPT: THE OXYGEN FAMILY Since the structure and organization of Group 6A mirrors that of Group 5A there will be many similarities between the two.

Group 5A

Group 6A

Similarities

N O

P S

As Se

Sb Te

Bi Po

Nh Lv


Allotropism

Oxygen (2 Major Forms) - ______ represents the more stable, safe form and is colorless as well as odorless.

- ______ represents the more hazard form and is bluish in color, while possessing a strong smell.

Sulfur (More than ______ different forms)

- The most stable allotrope is ____________________________.

SSS S

S SS S

Selenium (Se , Se2 , Se6, Se8 & Se10 )

Tellurium (2 Major Forms)

- Amorphous tellurium, which is either a blackish or dark grayish color.

- Crystalline tellurium, which possesses a hexagonal shape.



Page 14

CONCEPT: THE HALOGENS The halogens, elements in Group 7A, represent the last reactive group on the periodic table.

• The halogens exist as diatomic molecules: _______, _______, _______, _______ & _______.

• The final slot of the group belongs to ___________________, which was previously named __________________.


The halogens display predictable trends in their physical properties.

• Intermolecular force: _______________________________.

• As we move down the group there is a (n) _______________ in the strength of these intermolecular forces.

Group 7A

Bond Length (pm)

Bond Energy (kJ/mol)

Physical Features

F–F 143 159

Cl–Cl 200 243

Br–Br 228 193

I–I 266 151

Oxidation States

• Oxidation State: The _____ oxidation state is the most common and all the halogens except for _____ can obtain all the odd-numbered states from ______ to ______.

• Halogens react exothermically with one another to form interhalogen compounds. Ex: ____________

Halo-oxyanions

Oxyanion

Hypohalite __________

Halite __________

Halate __________

Perhalate __________

Fluorine

Chlorine

Bromine

Iodine

* In basic solutions halogens form hypohalites and at elevated tempeatures it can form halates.



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CONCEPT: ALLOYS

An alloy represents a _________________ mixture composed of two or more elements in which at least one of the elements is a metal.

• The predominant metal component, which is can be up to 90% or higher in terms of composition is referred to as the ____________ or ____________ metal.

• The minor components, which usually average around 1% in terms of composition, are referred to as the _______________________.

Alloys can be created by three different methods:

1) Heating the alloy components into liquids, mix them together and allowing them to cool into a ____________________.

2) ____________________ : turning the components into powders, mixing them together and allowing them to fuse.

3) ____________________: firing beams of ions at the surface of the host metal and allowing other components to mix.

Alloys are classified into two major types:

• A(n) _______________________ alloy is where some of the host metal atoms have been replaced by other metal atoms that have a similar size.

• A(n) _______________________ alloy is where the empty spaces between the host metal atoms have been taken up by smaller metal atoms.

Other common alloys that are good to remember include:

______________________ – copper (host metal), tin, manganese, phosphorus, aluminum, silicon.

______________________ – tin (host metal), copper, lead, antimony.

______________________ – iron (host metal), chromium with very small amounts of carbon, nickel, manganese & molybdenum.



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CHEMISTRY - BROWN 13E CH.22 - CHEMISTRY OF THE...

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