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Mobile App Chapter 8: Problem 8
Write formulas for each of the following compounds: a. potassium hydroxide b. calcium nitrate c. sodium carbonate d. carbon tetrachloride e. magnesium bromide
Short Answer
Expert verified
a. KOH, b. Ca(NO₃)₂, c. Na₂CO₃, d. CCl₄, e. MgBr₂
Step by step solution
01
Identify the Ions
For each compound, identify the cation (positive ion) and the anion (negative ion). This will help in writing the correct formula.
02
Write the Formula for Potassium Hydroxide
Potassium (K) has a +1 charge and hydroxide (OH) has a -1 charge. The formula is obtained by balancing these charges: KOH
03
Write the Formula for Calcium Nitrate
Calcium (Ca) has a +2 charge and nitrate (NO₃) has a -1 charge. To balance these charges, two nitrate ions are needed: Ca(NO₃)₂
04
Write the Formula for Sodium Carbonate
Sodium (Na) has a +1 charge and carbonate (CO₃) has a -2 charge. To balance the charges, two sodium ions are needed: Na₂CO₃
05
Write the Formula for Carbon Tetrachloride
Carbon tetrachloride is a molecular compound, consisting of one carbon atom covalently bonded to four chlorine atoms: CCl₄
06
Write the Formula for Magnesium Bromide
Magnesium (Mg) has a +2 charge and bromide (Br) has a -1 charge. To balance these charges, two bromide ions are needed: MgBr₂
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
ionic compounds
Ionic compounds are formed when elements transfer electrons to achieve a full outer shell, resulting in the formation of ions. These ions have positive (cation) and negative (anion) charges. For example, in potassium hydroxide (KOH), potassium (K) is the cation with a +1 charge, and hydroxide (OH) is the anion with a -1 charge. The resulting compound balances these charges, producing a stable ionic structure.
molecular compounds
Molecular compounds are formed when atoms share electrons through covalent bonds. This process leads to the formation of molecules rather than ions. An example is carbon tetrachloride (CCl₄), where one carbon atom shares electrons with four chlorine atoms, creating covalent bonds. Molecular compounds often have distinct properties such as lower melting points and the ability to form gases, unlike ionic compounds.
chemical charges
Chemical charges arise from the loss or gain of electrons by atoms. Cations are positively charged as they lose electrons, while anions are negatively charged as they gain electrons. For instance, magnesium (Mg) becomes a cation with a +2 charge upon losing two electrons, while bromide (Br) becomes an anion with a -1 charge upon gaining one electron. These charges are essential in forming stable compounds by balancing positive and negative forces.
balancing charges
Balancing charges is crucial in writing correct chemical formulas. The total positive charge must equal the total negative charge. For calcium nitrate (Ca(NO₃)₂), calcium (Ca) has a +2 charge, and nitrate (NO₃) has a -1 charge. To balance these charges, two nitrate ions are required to offset the +2 charge of one calcium ion, resulting in a balanced formula. This rule ensures the stability of ionic compounds.
cation
A cation is an atom or molecule with a net positive charge due to the loss of one or more electrons. Cations are typically metals like sodium (Na), which loses one electron to become Na⁺, or magnesium (Mg), which loses two electrons to become Mg²⁺. Cations are attracted to anions in ionic compounds, resulting in the formation of stable ionic bonds. The type and number of electrons lost determine the charge on the cation.
anion
An anion is an atom or molecule with a net negative charge due to the gain of one or more electrons. For example, bromine (Br) gains one electron to become Br⁻, while hydroxide (OH) is a polyatomic ion with a -1 charge. Anions pair with cations to form ionic compounds, maintaining the balance of charges. The process of gaining electrons and the resultant charge depend on the element's position in the periodic table and its tendency to attract electrons.
