Examples of ionic compound
1. Sodium chloride (NaCl)
2. Magnesium oxide (MgO)
3. Calcium carbonate (CaCO3)
4. Potassium iodide (KI)
5. Aluminum sulfate (Al2(SO4)3)
6. Iron(III) chloride (FeCl3)
7. Lithium nitrate (LiNO3)
8. Sodium hydroxide (NaOH)
9. Potassium bromide (KBr)
10. Calcium phosphate (Ca3(PO4)2)
Sure! Here are some examples of common ionic compounds:
1. Sodium chloride - NaCl
2. Calcium carbonate - CaCO3
3. Potassium iodide - KI
4. Magnesium oxide - MgO
5. Aluminum chloride - AlCl3
6. Iron(II) sulfate - FeSO4
7. Copper(II) sulfate - CuSO4
8. Silver nitrate - AgNO3
9. Ammonium sulfate - (NH4)2SO4
10. Barium chloride - BaCl2
Ionic compounds are formed when a metal reacts with a non-metal. In these compounds, the metal loses electrons to become a positively charged ion (cation), while the non-metal gains those electrons to become a negatively charged ion (anion). Here are some examples of common ionic compounds:
1. Sodium Chloride (NaCl): Sodium (Na) is a metal that loses an electron to form a sodium cation (Na+), while chlorine (Cl), a non-metal, gains that electron to become a chloride anion (Cl-). They combine in a 1:1 ratio to form sodium chloride.
2. Calcium Oxide (CaO): Calcium (Ca) donates two electrons to become a calcium cation (Ca2+), while oxygen (O) accepts those electrons to form an oxide anion (O2-). They combine in a 1:1 ratio to form calcium oxide.
3. Potassium Nitrate (KNO3): Potassium (K) loses one electron to become a potassium cation (K+), while nitrogen (N) and oxygen (O) in the nitrate ion accept those electrons. Nitrate (NO3-) is a polyatomic ion with a charge of -1. They combine in a 1:1:3 ratio to form potassium nitrate.
4. Magnesium Chloride (MgCl2): Magnesium (Mg) donates two electrons to form a magnesium cation (Mg2+), while chlorine (Cl) accepts those electrons to become a chloride anion (Cl-). They combine in a 1:2 ratio to form magnesium chloride.
These are just a few examples of ionic compounds. The naming and formulas of ionic compounds are determined by the charges of the ions and the ratio in which they combine.