Potassium and Calcium

What is an Atom?

The tiniest elements that constitute every matter cannot be broken down by chemical reaction. The tiniest component of an element that nonetheless exhibits elemental characteristics is called an atom. Everything in the cosmos, including ourselves, is made up of atoms. People often think of an atom as the smallest possible form of matter, but even smaller particles make up an atom.

Atomic Structure

• The nucleus is the dense core of each atom.
• Neutrons, which have a neutral electric charge, and protons, which have positive charges, make up the nucleus.
• The physical characteristics of an element are determined by the number of protons in an atom. There are different numbers of protons in each element.
•  The negatively charged particles known as electrons orbit the nucleus like planets orbit the sun.
• Protons and electrons are pulled towards one another and are typical of equal numbers.
• The amount of the proton and neutron contained in the nucleus is the atomic mass unit.
  For instance, the helium atom has an atomic number of 4 because it has 2 protons and 2 neutrons in its nucleus.

Potassium

1. About Potassium

• Due to the fact that potassium is a chemical element, it cannot be subdivided by chemical processes. There are several of the same atoms in it.
• The word "potash," which describes the kind of potassium-rich fertilizer that farmers used to manufacture from pot ash, is where the word "potassium" originates.
• The name Kalium, which comes from the Latin term alkali, which means soda ash, is another name for potassium. Due to its other name, Kalium, potassium is designated as K in the periodic table.
• Potassium belongs to the group of delicate, silver-white metals known as alkali metals.
• Due to its high reactivity, potassium frequently loses its solitary valent electron when it is combined with other elements.

2. Isotopes

• Atoms of the same element can have an extra neutron. These are called isotopes.
• Isotopes maintain their elemental chemical characteristics while having varied neutron counts because the proton count stays constant.
• Only three potassium isotopes are known to be stable.
  • Potassium 39
    • Nineteen electrons, 19 protons, and 20 neutrons make up the atom.
    • On the periodic table, this is the form that can be found.
    • This isotope makes up 93.3 percent of all the potassium that may be found in nature.
  • Twenty-one neutrons in potassium 40
  • Twenty-two neutrons in potassium 41. It is the isotope in the rarest form.

3. Atomic Structure

• Atomic number: 19
• Atomic Code: K
• It is a metal categorized as an alkali.
• It belongs to period four of the periodic table.
• Its nucleus has 20 neutral neutrons and 19 positively charged protons.
• To counteract its 19 positively charged protons, it possesses 19 negatively charged electrons.
• Four orbital shells around the nucleus contain electrons.

4. Physical properties

• It is an element of alkali.
• It has a silvery gloss and is delicate and white.
• Potassium metal's melting point is low.
• It is good for heat and electricity transport.
• Gives a flame a purple hue, and its vapor is green.
• The commonly diagnosed element in the crust of the planet
• This metal is malleable.

5. Chemical properties

• Potassium devalues when it encounters air and water. Superoxide of potassium is produced when potassium burns in the air.
• Water and potassium quickly respond to produce potassium hydroxide and hydrogen gas in the form of a colourless solution.
• Potassium forms potassium halides when it combines with halogens.
• Potassium forms the K ion with hydrogen gas when it dissolves in diluted sulfuric acid.

6. Uses

• It is an effective fertilizer.
• It serves as a substitute for salt.
• Used in detergents and soaps
• Pyrotechnics
• All plants and animals require it. It is necessary for photosynthesis, growth, osmosis control, and enzyme activation in plants. Animals have carefully controlled their potassium levels.

Calcium

1. About Calcium

1. Calcium has the chemical symbol Ca.
2. The English, Greek, or Latin names of the elements are used as their chemical symbols.
3. The Latin word calx or calcis, which means limestone, is where the name calcium comes from.

2. Isotopes

• From 34Ca to 60Ca, there are twenty-seven isotopes of calcium.
• There are only five stable isotopes, though (40, 42, 43, 44, and 46). Both the common isotope 40Ca and the uncommon 46Ca are theoretically unstable. The radioactive isotope is 41Ca.

3. Atomic Structure

• The atomic numberis 20.
• It has 20 electrons or negatively energetic particles.

4. Physical properties

• Each element has observable and quantifiable physical characteristics, such as density, color, and smell.
• It is a metallic element that is solid, silvery, and fairly hard.
• It ranks as the sixth most prevalent element on the planet.
• The silvery white metal is the color.
• Phase: Solid
• Cubic crystal structure
• Ductility: It is capable of being formed into very thin sheets.
• It is malleable and may be bent or moulded.
• Hardness: This metal is rather mild.

5. Chemical properties

• They are the qualities that control how the substance will interact with elements like oxygen or water.
• Flammability: It ignites when heated in air or oxygen.
• Incompatibility with water: It quickly reacts with cold water initially, but when a calcium hydroxide coating forms, the reaction eventually slows down.
• Extremely sensitive to acids
• Deoxidizer used in steel to prevent oxidation

6. Uses

• In the construction sector, calcium compounds like gypsum, marble, chalk, and limestone are employed.
• In concrete
• Whitening powder
• Using metallic calcium, steel is deoxidized.