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NaCl is an ionic compound. Na ions are positive charged and Cl ions are negative charged. A Coulomb force is existing between the two kinds of ions, making NaCl an ionic compound.
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What is the molecular equation complete ionic equation and the net ionic equation for NaCl Na2CO3?
These two compounds doesn't react.
Are all compounds composed of molecule's?
some compounds are composed of molecules bound by ionic compounds so no
What are the two major types of compounds?
There are two types of compounds: molecular and ionic. ill give you an example of each Water-H20 molecular compound Salt-NaCl ionic compoundThere are ionic compounds which is a compound formed by a positive metal ion and a negative nonmetal ion. And there are convalent compounds which is a compound formed in which atoms share electrons.
What are two kinds of compounds?
The two types of compound are molecular and ionic. An ionic compound commonly used is table salt, or NaCl. A molecular compound commonly used is water, or H2O.
Do ionic compounds and molecular compounds behave similarly when they are dissolved?
Ionic compounds eg NaCl yield ions when dissolved in water, NaCl (in water) -> Na positive ions and negative Cl ions. Ions have electrical charges & conduct electricity. All compounds are "molecular", ie they are made up of more than one atom in combination. Some molecules are not ionic, eg common sugar, and when they are dissolved in water they do not yield ions and do not conduct electricity.
Molecular compounds boil at much higher temperatures than do ionic compounds true or false?
This is false. Ionic compounds have higher boiling points than molecular compounds. For example, the boiling point of the ionic compounds copper(II) oxide, CuO, and sodium chloride, NaCl are 2,000 degrees C and 1,413 degrees C, respectively. The boiling point of the molecular compounds carbon tetrachloride, CCl4, and water, H2O are 76.72 degrees C and 100 degrees C, respectively.
How do ionic and molecular compounds differ in physical properties?
Ionic compounds have higher melting and boiling points than molecular compounds due to the strong electrostatic forces between ions. Ionic compounds are usually solid at room temperature, while molecular compounds can be solid, liquid, or gas. Ionic compounds conduct electricity when dissolved in water, while molecular compounds do not.
What compounds has an ionic bond SO3 CO2 NaCl HCl?
SO3 does not form ionic bonds; it forms covalent bonds. CO2 also forms covalent bonds due to its molecular structure. NaCl and HCl both have ionic bonds because they are formed between a metal (Na) and a nonmetal (Cl) in NaCl, and a metal (H) and a nonmetal (Cl) in HCl.
What compounds exhibit ionic bonding?
NaCl
How many types of compound are there and name?
There are two main types of compounds: molecular compounds and ionic compounds. Molecular compounds are formed by sharing electrons between atoms, while ionic compounds are formed through the transfer of electrons between atoms. Examples of molecular compounds include water (H2O) and carbon dioxide (CO2), while examples of ionic compounds include sodium chloride (NaCl) and potassium iodide (KI).
How can molecular compounds be distinguished from ionic compounds?
Molecular compounds are formed by sharing electrons between atoms to create covalent bonds, while ionic compounds are formed by transferring electrons from one atom to another to create ionic bonds. Molecular compounds typically have lower melting and boiling points compared to ionic compounds, which have high melting and boiling points due to strong electrostatic forces between ions. Molecular compounds are typically composed of nonmetals, while ionic compounds are composed of metals and nonmetals.
How can water dissolve some ionic compounds as well as some molecular compounds?
Water can dissolve some ionic compounds as well as some molecular compounds because of its polarity. It is polar enough to dissolve ionic compounds into their ions. Water does not dissolve molecular compounds by breaking covalent bonds, but through intermolecular forces.
