Chemical Reactions Overview
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Questions and Answers

What is the difference between gypsum and barite?

  • Barite is $BaSO_4$ (correct)
  • Gypsum is found in nature (correct)
  • Gypsum is used in making Plaster of Paris (correct)
  • Gypsum is $CaSO_4.2H_2O$ (correct)

How can we get rid of excess $CO_2$?

By reacting calcium hydroxide with carbon dioxide, we get calcium carbonate and water. $Ca(OH)_2 + CO_2 -> CaCO_3 + H_2O$. This converts carbon dioxide into calcium carbonate.

Flashcards

Gypsum

A mineral composed of calcium sulfate dihydrate (CaSO₄·2H₂O), commonly used in construction materials.

Plaster of Paris

A white powder made from gypsum (CaSOâ‚„) that sets into a hard solid when mixed with water, used for plastering and sculptures.

Calcium Hydroxide

A chemical compound with the formula Ca(OH)â‚‚, also known as slaked lime, used for detecting COâ‚‚ and in cement production.

Sodium

A soft, silvery-white alkali metal that is highly reactive and not found freely in nature.

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Reducing Agent

A substance that donates electrons to another substance, causing it to gain electrons and be reduced.

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Sodium Chloride

A compound with the chemical formula NaCl, commonly known as table salt.

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Hygroscopic

A substance that absorbs moisture from the air, becoming damp.

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Sodium Hydroxide

A strong base with the formula NaOH, also known as caustic soda, used in many industrial processes.

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Calcium Oxide

A white solid with the formula CaO, also known as quicklime.

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Alkali Metals

Elements in group 1 of the periodic table, highly reactive and found in alkaline solutions.

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Alkaline Earth Metals

Elements in group 2 of the periodic table, less reactive than alkali metals.

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Electronegativity

A measure of the atom's ability to attract electrons in a chemical bond.

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Ionization Energy

The energy required to remove an electron from an atom.

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Valence Electron

An electron in the outermost shell of an atom, responsible for chemical bonding.

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Reducing Agent

A substance that loses electrons in a chemical reaction, causing another substance to gain electrons and be reduced.

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Sodium

A highly reactive alkali metal, not found free in nature, used in many industrial processes.

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Atomic Number

The number of protons in an atom's nucleus, defining the element.

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Atomic Mass

The average mass of an atom of an element, taking into account isotopes.

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Electron Configuration

The arrangement of electrons in an atom's energy levels or orbitals.

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Flame Test

A technique used to identify elements based on the color of the flame they produce when heated.

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Lithium

The lightest alkali metal, found in batteries.

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Sodium

A soft, silvery-white alkali metal, found in table salt, and used in many industrial processes.

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Potassium

A highly reactive alkali metal, found in bananas and fertilizers.

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Calcium

An alkaline earth metal found in bones, teeth, and milk.

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Magnesium

An alkaline earth metal found in chlorophyll and magnesium ribbon.

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Beryllium

The lightest alkaline earth metal, found in certain alloys.

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Strontium

An alkaline earth metal used in fireworks, producing a red color.

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Barium

An alkaline earth metal used in X-ray imaging.

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Study Notes

Chemical Reactions

  • Chemical reactions involve the rearrangement of atoms to form new substances.
  • Reactants are the substances that undergo a chemical change.
  • Products are the new substances formed as a result of the chemical change.
  • The general equation for a chemical reaction is : Reactants → Products
  • Chemical equations represent the reactants and products and their relative quantities.
  • Chemical equations are balanced to ensure the law of conservation of mass (that matter cannot be created nor destroyed).

Examples of Chemical Reactions

  • Calcium hydroxide (Ca(OH)2) reacts with carbon dioxide (CO2) to form calcium carbonate (CaCO3) and water (H2O).
    • Ca(OH)2 + CO2 → CaCO3 + H2O
  • Calcium sulfate dihydrate (CaSO4.2H2O) can decompose to form calcium sulfate (CaSO4) and water (H2O).
    • CaSO4.2H2O → CaSO4 + 2H2O

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Description

This quiz covers the basics of chemical reactions, including the definitions of reactants, products, and the importance of balancing chemical equations. Explore how substances interact and transform into new products through various examples. Test your understanding of the fundamental principles that govern chemical changes.

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