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Inorganic Chemistry Homework Help

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What Is Inorganic Chemistry? How Does It Differ From Organic Chemistry?

Inorganic chemistry is a branch of chemistry that deals with the interactive patterns and synthesis of inorganic and organometallic compounds. The chemistry unit is usually about all the inorganic sections, with the organic chemistry section excluded.

Organic compounds feature carbon atoms that covalently bond to hydrogen atoms. On the other hand, inorganic compounds have many elements that do not have carbon.

That said, inorganic chemistry is about compounds without carbon. The inorganic chemistry section studies the reactions of elements and compounds that do not contain carbon atoms usually associated with organic chemistry.

Inorganic chemistry is vital in many practical technologies, such as:

• Energy conversion and storage

• Catalysis and structural, electronic, magnetic, and other materials

• Productions of nylons, plastics, and fiber

Branches of Inorganic Chemistry

According to our expert tutors, there are various branches of inorganic chemistry:

1. Inorganic solid-state chemistry

2. Main group elements in inorganic chemistry

3. Transition metal complexes

4. Coordination chemistry

5. Bioinorganic chemistry

6. Materials science

7. Geochemistry

8. Nuclear science and energy

9. Synthetic inorganic chemistry

10. Reaction kinetics and mechanisms

11. Organometallic compounds

12. Inorganic technology

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Inorganic Chemistry Homework Help for Different Classifications

There are various classifications of inorganic chemical compounds. Our inorganic chemistry assignment help will help you know all the categories and operations of the compounds. The various substances you will study in inorganic chemistry include:

1. Acids

Acids are compounds that usually dissolve in water to form hydrogen ions. A good example is a sulphuric acid, hydrogen chloride acids, vinegar, etc.

2. Bases

Bases are substances that produce hydroxyl ions when you expose them to water. A good example may be sodium hydroxide, ammonia, etc.

3. Salts

You will always get the formation of salts when acids and bases react. E,g, sodium chloride.

4. Oxides

Oxides are compounds consisting of one oxygen atom.

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Types of Chemical Reactions Covered in Inorganic Chemistry Assignments

You will be expected to cover various chemical reactions in any chemistry assignment.

Our tutors will help you understand displacement reactions, acid-base reactions, and redox reactions, usually tough nuts to crack in inorganic chemistry.

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Here are some types of chemical reactions that our experts will help you with:

1. Combination Reaction

When you put two or more elements together, they usually react to form compounds. For example, sulfur and iron come together to produce iron sulfate.

2. Decomposition Reaction

This type of reaction is the opposite of a combination reaction. In decomposition reactions, compounds break down into smaller molecules or elements.

For example, it breaks down into calcium oxide and carbon dioxide when you heat calcium carbonate.

3. Displacement Reaction

In displacement reactions, one element displaces another from a compound. For example, when you mix sodium and potassium chlorides, potassium will displace out of the compound since it is more reactive than sodium.

4. Acid-Base Reactions

In acid-base reactions, acids and bases interact to produce salts and water. For example, when you mix hydrochloric acid with sodium hydroxide, they react to form sodium chloride and water.

5. Redox Reactions

Redox reactions involve the transfer of electrons between molecules. In these reactions, one molecule becomes oxidized while another becomes reduced.

An excellent example of a redox reaction is the rusting of iron. Iron is oxidized to form rust (iron oxide).

6. Catalytic Reactions

Catalytic reactions are chemical reactions that are sped up by catalysts. A catalyst is a molecule that is not consumed in the reaction.

For example, platinum is a catalyst used to convert hydrogen into helium in nuclear reactors.

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Descriptive Inorganic Chemistry

Descriptive inorganic chemistry is generally concerned with identifying unknown compounds, using mainly physical methods.

1. Main group Compounds

They are usually based on groups one, two, 13, and 18 of the periodic table.

2. Coordination Compounds

Coordination compounds are lone electrons pairs that fall under the atomic groups and contain features of metals within them.

All organic and inorganic compounds are essential to be used as a substance. Every metal here is from group 3 to 13.

3. Transition Metal Compounds

The group has metallic compounds from four to eleven in the periodic table. However, there may be an addition of groups three to twelve at times. With that, you will get a superb coordinating relation between all the elements.

4. Organometallic Compounds

They are compounds with M-C-H groups in them. Here, the metals can have the transition or main group elements. High lipophilic complexes are usually available with metals, alkoxides, and carbonyls.

Other than the compounds above, there are also other compounds that you can get homework and assignment help services in. They may be bioinorganic compounds, cluster compounds, or even solid-state compounds.

Examples of Questions in Inorganic Chemistry

1. How many coordination compounds can you make with the following: [Co(NH)(H2O)4]Cl-?

There are four; one of NH3, NH4+, and two water molecules.

2. The element in group 3 is _________ and has an atomic radius of 0.07 nm.

The element is lithium and has an atomic radius of 0.07 nm.

3. What type of compound is CrCl3?

CrCl3 is a coordination compound.

4. Draw the Lewis structure for phosphorus pentachloride, PCl5.

PCl5 has 5 Cl atoms and 1 P atom. There is one lone pair on the P atom, so 5 Cl atoms surround it. The Lewis structure is:

5. How many unpaired electrons are in Fe2O3?

There are 3 unpaired electrons in Fe2O3.

6. Identify the oxidation state of chromium in CrCl3.

The oxidation state of chromium in CrCl3 is +3.

7. Which atoms are isoelectronic with O?

Oxygen and sulfur are both isoelectronic with oxygen and have similar electronic structures, so they may be used to help solve the problem:

Theories You Will Learn in Inorganic Chemistry

Inorganic chemistry is a vast subject with many theories and concepts that students need to learn. In general, these are the main theories that you will learn in inorganic chemistry:

Brønsted–Lowry theory

The theory is based on the concept that a proton donor is a Brønsted acid and a proton acceptor is a Brønsted base.

Aqueous solutions of strong acids such as hydrochloric acid and sulfuric acid are good Brønsted–Lowry acids because they freely donate protons (H+).

On the other hand, aqueous solutions of strong bases such as sodium hydroxide and potassium hydroxide are good Brønsted–Lowry bases, because they accept protons (H+) freely.

Lewis theory

The theory is based on the concept that every chemical bond is established by electrons. A covalent bond can be formed when two atoms simultaneously share one pair of electrons.

For example, oxygen (O) has an octet and it will establish a strong covalent bond when it shares its electron with another atom.

The two atoms are then held together by this new covalent bond.

A Lewis acid is an electron pair acceptor, while a Lewis base is an electron-pair donor.

For example, O can be considered a Lewis base because it has one empty orbital that allows it to share its electron pair with another atom.

Valence bond theory

The Valence Bond Theory is a model that explains the arrangement of electron pairs in chemical bonds. It states that covalent bond formation is due to overlapping atomic orbitals, which are filled with electrons.

For example, methane (CH) forms four covalent C-H bonds because each hydrogen atom contributes one electron to the carbon atom, which uses its four outer electrons to establish four covalent bonds.

This theory is also known as the "octet rule" because every atom in a molecule wants eight electrons in its valence shell. If an atom doesn't have this number of electrons in its valence shell, it will share electrons with other atoms to achieve this octet.

Molecular orbital theory

The Molecular Orbital Theory is a model that explains the arrangement of electron pairs in molecules. It states that covalent bond formation is due to the overlap of atomic orbitals, which creates new molecular orbitals.

These molecular orbitals can be either bonding or antibonding.

A bonding molecular orbital allows the electrons to be shared between two atoms. In contrast, an antibonding molecular orbital does not allow the electrons to be shared between two atoms.

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Answer Application Questions in Inorganic Chemistry

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