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Chapter 2: Problem 102

Give the chemical names of each of the following familiar compounds: (a) \(\mathrm{NaCl}\) (table salt), (b) \(\mathrm{NaHCO}_{3}\) (baking soda), (c) \(\mathrm{NaOCl}\) (in many bleaches), (d) \(\mathrm{NaOH}\) (caustic soda), (e) (NH \(_{4}\) ) \(_{2} \mathrm{CO}_{3}\) (smelling salts), (f) \(\mathrm{CaSO}_{4}\) (plaster of Paris).

Short Answer

Expert verified
The chemical names for the given compounds are: (a) Sodium Chloride, (b) Sodium Bicarbonate, (c) Sodium Hypochlorite, (d) Sodium Hydroxide, (e) Ammonium Carbonate, and (f) Calcium Sulfate.

Step by step solution

01

(a) Name of NaCl

The compound NaCl is composed of one sodium ion (Na+) and one chloride ion (Cl-). Thus, the chemical name for NaCl is Sodium Chloride.
02

(b) Name of NaHCO3

The compound NaHCO3 is composed of one sodium ion (Na+) and one bicarbonate (HCO3-) ion. Thus, the chemical name for NaHCO3 is Sodium Bicarbonate.
03

(c) Name of NaOCl

The compound NaOCl is composed of one sodium ion (Na+) and one hypochlorite (OCl-) ion. Thus, the chemical name for NaOCl is Sodium Hypochlorite.
04

(d) Name of NaOH

The compound NaOH is composed of one sodium ion (Na+) and one hydroxide (OH-) ion. Thus, the chemical name for NaOH is Sodium Hydroxide.
05

(e) Name of (NH4)2CO3

The compound (NH4)2CO3 is composed of two ammonium ions (NH4+) and one carbonate (CO3^2-) ion. Thus, the chemical name for (NH4)2CO3 is Ammonium Carbonate.
06

(f) Name of CaSO4

The compound CaSO4 is composed of one calcium ion (Ca^2+) and one sulfate (SO4^2-) ion. Thus, the chemical name for CaSO4 is Calcium Sulfate.

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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 atoms transfer electrons from one to another, resulting in ions. These ions are oppositely charged and thus experience electrostatic attractions, binding them together to form a compound.
In ionic compounds, metals typically lose electrons to become positively charged cations, while non-metals gain electrons to become negatively charged anions.
This transfer creates stability through fulfilling the octet rule, where atoms aim to have eight electrons in their valence shell, similar to noble gases.
  • An example is sodium chloride (\( \text{NaCl} \)), where sodium (Na) transfers one electron to chlorine (Cl), forming \( \text{Na}^+ \) and \( \text{Cl}^- \) ions.
  • Ionic compounds are generally solids at room temperature and have high melting and boiling points due to the strong forces holding the ions together.
  • They also tend to dissolve well in water, creating solutions that can conduct electricity.
Understanding ionic compounds is fundamental in chemical nomenclature, as it helps in naming and recognizing various substances by identifying the ions involved.
Chemical Formulas
Chemical formulas provide a means of conveying information about the composition of molecules and ionic compounds. These formulas use the element symbols from the periodic table and numerical subscripts to depict the number of atoms of each element.
For ionic compounds, the chemical formula represents the ratio of ions that result in a neutral compound.
Take, for example, the formula for baking soda, \( \text{NaHCO}_3 \) , which reflects the presence of one sodium ion, one hydrogen ion, and one carbonate ion.
  • Chemical formulas are critical for understanding the makeup and properties of a substance.
  • They must balance the charges of the ions to maintain electrical neutrality in the compound.
  • In the formula \( \text{(NH}_4\text{)}_2\text{CO}_3 \) , there are two ammonium ions \( \text{(NH}_4^+) \) for every one carbonate ion \( \text{CO}_3^{2-} \) , ensuring the entire compound remains neutral.
These formulas are foundational in chemical equations and reactions, serving as the basic language of chemistry.
Ion Identification
Ion identification is a crucial part of chemical nomenclature, allowing chemists to deduce the names of compounds. Identifying ions involves recognizing whether an ion is a cation or an anion and understanding its charge.
Ions are often part of larger compounds and can frequently exist in multiple forms depending on their environmental conditions and interactions with other ions.
Polyatomic ions, such as sulfate \( \text{SO}_4^{2-} \) , play significant roles in many compounds like \( \text{CaSO}_4 \) .
  • Cations like sodium \( \text{Na}^+ \) are identified by their ability to lose electrons and form positive charges.
  • Anions like chloride \( \text{Cl}^- \) are identified by their ability to gain electrons and form negative charges.
  • Polyatomic ions are groups of covalently bound atoms that carry a charge, such as bicarbonate \( \text{HCO}_3^- \) , which is essential in the formation of baking soda.
Recognizing these ions, their charges, and how they combine is essential for writing and interpreting chemical formulas and names correctly.

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Most popular questions from this chapter

Many familiar substances have common, unsystematic names. For each of the following, give the correct systematic name: (a) saltpeter, \(\mathrm{KNO}_{3} ;\) (b) soda ash, \(\mathrm{Na}_{2} \mathrm{CO}_{3} ;\) (c) lime, \(\mathrm{CaO}\); (d) muriatic acid, \(\mathrm{HCl}\); (e) Epsom salts, \(\mathrm{MgSO}_{4}\); (f) milk of magnesia, \(\mathrm{Mg}(\mathrm{OH})_{2}\).

The elements of group 4 A show an interesting change in properties moving down the group. Give the name and chemical symbol of each element in the group, and label it as a nonmetal, metalloid, or metal.

An \(\alpha\) particle is the nucleus of an \({ }^{4} \mathrm{He}\) atom. (a) How many protons and neutrons are in an \(\alpha\) particle? (b) What force holds the protons and neutrons together in the \(\alpha\) particle? (c) What is the charge on an \(\alpha\) particle in units of electronic charge? (d) The charge- to-mass ratio of an \(\alpha\) particle is \(4.8224 \times 10^{4} \mathrm{C} / \mathrm{g}\). Based on the charge on the particle, calculate its mass in grams and in amu. (e) By using the data in Table 2.1, compare your answer for part (d) with the sum of the masses of the individual subatomic particles. Can you explain the difference in mass? (If not, we will discuss such mass differences further in Chapter 21.)

Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of \(\mathrm{H}_{2}\) is taken under conditions that prevent decomposition into \(\mathrm{H}\) atoms. The two naturally occurring isotopes of hydrogen are \({ }^{1} \mathrm{H}\) (atomic mass \(=1.00783\) amu; abundance \(99.9885 \%\) ) and \({ }^{2} \mathrm{H}\) (atomic mass \(=2.01410 \mathrm{amu}\); abundance \(0.0115 \%\). (a) How many peaks will the mass spectrum have? (b) Give the relative atomic masses of each of these peaks. (c) Which peak will be the largest, and which the smallest?

Determine whether each of the following statements is true or false. If false, correct the statement to make it true: (a) The nucleus has most of the mass and comprises most of the volume of an atom; (b) every atom of a given element has the same number of protons; (c) the number of electrons in an atom equals the number of neutrons in the atom; (d) the protons in the nucleus of the helium atom are held together by a force called the strong nuclear force.
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