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Transcript

Oxides

14.04.2022

Maja HSIB

Agenda

1. What are oxides?

- how we divide them

Agenda

2. Types (groups) of oxides.

3. Examples of oxides that are present in our daily lives.

Oxides

Oxide is a combination of oxygen with any element. Oxygen combines with metals and non-metals. Important: Oxygen in oxides is (mostly) in the -II oxidation state, it is bivalent.

*exceptions:

- OF 2 +II

H2O -II

H2O2 -I

NaO2 -1/2

Metals and nonmetals

Oxides of metals and nonmetals

Lithium and beryllium metals form one type of oxide. Lithium are always mono-valent, while Beryllium is divalent.

Non-metals form several types of oxides. It depends on the valence of the non-metal. Important: the valency of the non-oxide-forming metal is compulsory, which means that for example, we cannot say nitric oxide because Nitrogen makes up five oxides.

Oxide groups

Oxide groups

1. Acid oxides,

2. Basic oxides

3. Atmospheric oxides,

4. Neutral oxides.

Acid oxides

1.

- these are compounds in which a non-metal atom is connected with oxygen. They do not react with strong acids, but with strong bases. They dissolve in water. An example is acid anhydrides.

SO2

SO3

CO2

Basic oxides

2.

- are compounds of oxygen with the metal. They react with strong acids but not bases. They dissolve in water, for example alkali and alkaline earth oxides.

MnO

HgO

Amphoteric oxides

3.

- they react with strong acids and bases. They do not dissolve in water, examples are AL2O3, ZnO, Fe2O3.

Al2O3

ZnO

Fe2O3

Neutral oxides

4.

- do not react with water, acids or bases.

Examples: NO, CO, SiO

Physical properties

Physical properties

1. Solids - metal oxides,

2. Gases - non-metal oxides,

3. High melting point,

4. Water solubility,

5. High density.

How to get oxides?

Direct synthesis of two elements:

2Cl2 +5O2 -> 2Cl2O5

Oxidation of the oxide at a lower oxidation state:

2NO + O2 -> 2NO2

Reduction of the oxide at a higher oxidation state:

Fe2O3+ C -> FeO+ CO2

Fe2O3+H2 -> FeO + H2O

Thermal decomposition:

CaCO3 -> CaO +CO2

Burning organic compounds:

CH4+ 2O2 -> CO2 + 2H2O

Examples of oxides part.1

Examples of oxides I

H2O - Dihydrogen monoxide

SiO2 - Silicon dioxide

CO2 - Carbon dioxide

CO - Carbon monoxide

N2O - Nitrous oxide

Water - Dihydrogen monoxide

H2O

Water covers about 70% of our planet, Earth.

Living organisms like humans are mostly made of water.

It exists in three states (solid, liquid and gaseous) and does not have any taste, smell or color.

Humans and animals need water to live. Research shows that we can only survive couple of days without it.

H2O is also used for making food, dissolve various substances and recreational purposes.

Photo & Lewis structure

Silicon dioxide (silica)

SiO2

The chemical compound SiO2 occurs naturally in nature. It is the main component of sand.

In the natural environment, we can often find many varieties such as: rose, white, blue and green quartz, as well as citrine quartz, amethyst and mountain crystal.

It is acidic in nature because it reacts with an alkaline substance.

It is primarily used in the production of glass. Glass is a non-crystalline substance, which means that it is not structured in an orderly manner.

Photo & Lewis structure

Carbon dioxide

CO2

CO2 is a gas at standard conditions but heavier than air. It is odorless and colorless oxide and it is not toxic to humans. Carbon dioxide is soluble in water.

This oxide occurs naturally: the breath of animals, plants decay, vulcanos and also in human sources burning of fossils fuels, oil and natural gas.

We use CO2 for chemical, oil and food industry. The most known use of carbon dioxide is the production of carbonate beverages for instance beer or soda water.

Photo & Lewis structure

Carbon monoxide

CO

It is a gas without taste, smell or color. It is highly dangerous to people. It burns in air with a bright blue flame and is soluble in water at 20C degrees.

It is used for pharmaceutical manufacture, fuel gas mixtures with hydrogen and other gases for industrial and domestic heating.

This oxide is found in fumes, small engines, stoves, lanterns, grills, fireplaces, gas ranges, or furnaces.

Symptoms of poisoning; headache, weakness, upset stomach, vomiting and chest pain.

Lewis structure

Nitrous oxide

N2O

Nitrous oxide is a gas heavier than air. It does not have color or taste but it has an odor which can be described as slightly sweet. It is soluble in water.

It is known as laughing gas because of its intoxicating effects when inhaled. It is used for pharmacological agent to produce anesthesia, a food additive as a propellant or an additive to fuels to increase available oxygen in combustion.

It naturally occurs in soils under natural vegetation, tundra and the oceans.

Photo & Lewis structure

Example of oxides pt. II

Example of oxides II

SO2 - Sulfur dioxide

CaO - Calcium oxide

Ag2O - Silver oxide

Al2O3 - Aluminum oxide

Sulfur dioxide

SO2

SO2 is a gas heavier than air. It does not have a color but it has a pungent smell. While inhaled it can irritate eyes and mucous membranes, so it is toxic to humans. It dissolves in water.

It occurs while burning coal or oil at power plants but also forms copper smelting. Naturally it can be released to the air from volcanic eruptions.

It is used as a food bleaching agent, an Escherichia coil metabolite and a refrigerant.

Photo & Lewis structure

Calcium oxide

CaO

Calcium oxide is a solid. It does not have any smell but it has color. CaO is white or greyish.

It is produced in large quantities roasting calcium carbonate. It absorbs carbon dioxide from the atmosphere as well as water converting itself into calcium hydroxide and releasing heat in the process. The reaction of quicklime with water is used in portable heat sources.

Quicklime is used extensively as a building material or as a fertilizer

Large quantities of quicklime are used in various industrial neutralization reactions.

Photo & Lewis structure

Silver oxide

Silver oxide is a solid. It is a dark brown or black compound but it does not have an odor. Its crystal structure is cubic. It is soluble in water but its solubility increases with the temperature. Ag2O is also a harmful and toxic oxide. (if swallowed)

It is used in silver oxide batteries, synthesis of many compounds, it is suitable for ceramic, and optic applications also its applications are being studied in aerospace and fuel cells as well.

Ag2O

Photos & Lewis structure

Aluminum oxide

Aluminum oxide is a crystalline powder. It does not have any smell but it has white color. It is not soluble in H2O.

It is amphoteric in nature, occurring in nature as various minerals such as bauxite, corundum, etc.

It is used in various chemical, industrial and commercial applications. For instance: as an adsorbent, desiccating agent, and catalyst, and in the manufacture of dental cements and refractories.

Al2O3

Photo & Lewis structure

Sources

Sources

Books

- "biomedica - chemia zbiór zadań maturalnych 2022"

- "Greg - repetutorium maturzysty chemia"

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https://www.nhm.ac.uk/discover/quick-questions/where-does-carbon-dioxide-come-from.html#:~:text=Carbon%20dioxide%20(CO2)%20comes,natural%20gas%20to%20generate%20energy).

https://www.nyruralwater.org/sites/default/files/Winters_Summer%202020.pdf

https://pubchem.ncbi.nlm.nih.gov/compound/Carbon-dioxide

https://docs.google.com/document/d/1zcY6XUNbvH-PO8Mhyu6fjI4KrpB7sAFh74FToZXGUXA/edit?pli=1

https://www.cdc.gov/co/faqs.htm#:~:text=Where%20is%20CO%20found%3F,%2C%20gas%20ranges%2C%20or%20furnaces.

https://www.atsdr.cdc.gov/ToxProfiles/tp201-c4.pdf

https://www.linde-gas.com/en/products_and_supply/packaged_chemicals/product_range/carbon_monoxide.html

https://learn.kaiterra.com/en/air-academy/carbon-dioxide

https://pubchem.ncbi.nlm.nih.gov/compound/Nitrous-oxide

https://www.cornerstonedentistrybrantford.ca/site/blog/2016/04/05/a-brief-history-of-happy-gas-nitrous-oxide#:~:text=Nitrous%20Oxide%20is%20also%20called,and%20carbon%20dioxide%20among%20others).

https://pubchem.ncbi.nlm.nih.gov/compound/Sulfur-dioxide

https://www.britannica.com/science/calcium/Compounds#ref89814

https://www.vedantu.com/chemistry/silver-oxide

https://pubchem.ncbi.nlm.nih.gov/compound/Aluminum-oxide

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