Ionic Compounds

Review

Review The reactivity of an atom is primarily dependent on the valence shell

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways:

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons By losing electrons

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons By losing electrons The process of gaining or losing electrons is referred to as ionization

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons By losing electrons The process of gaining or losing electrons is referred to as ionization Atoms who have lost or gained an electron are called ions

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons By losing electrons The process of gaining or losing electrons is referred to as ionization Atoms who have lost or gained an electron are called ions Positively charged ions are called cations

Review The reactivity of an atom is primarily dependent on the valence shell If the valence shell is full, the atom is non-reactive For example: the noble gases The easier it is to fill the shell, the more reactive the atom will be For example: sodium (1 valence electron) will be more reactive than magnesium (2 valence electrons) because it is easier to give up one electron than two The valence shell can be filled in two ways: By gaining electrons By losing electrons The process of gaining or losing electrons is referred to as ionization Atoms who have lost or gained an electron are called ions Positively charged ions are called cations Negatively charged ions are called anions

Review For example: Sodium

Review For example: Sodium One valence electron

Review For example: Sodium One valence electron Easiest way to have a full valence shell is to lose this one electron

Review For example: Sodium One valence electron Easiest way to have a full valence shell is to lose this one electron After losing the electron, sodium will have an ionic charge of 1+ because it has one more proton than electron

Review For example: Fluorine

Review For example: Fluorine Seven valence electrons

Review For example: Fluorine Seven valence electrons Easiest way to fill valence shell is to gain one electron

Review For example: Fluorine Seven valence electrons Easiest way to fill valence shell is to gain one electron After gaining one electron, fluorine will have an ionic charge of 1-

What happens when an atom of sodium is put next to an atom of fluorine?

What happens when an atom of sodium is put next to an atom of fluorine? Fluorine is happy to accept the electron sodium wants to give up

What happens when an atom of sodium is put next to an atom of fluorine? Fluorine is happy to accept the electron sodium wants to give up

What happens when an atom of sodium is put next to an atom of fluorine? Fluorine is happy to accept the electron sodium wants to give up

What happens when an atom of sodium is put next to an atom of fluorine? After sodium gives its valence electron to fluorine, sodium will have a positive charge and fluorine will have a negative charge

What happens when an atom of sodium is put next to an atom of fluorine? After sodium gives its valence electron to fluorine, sodium will have a positive charge and fluorine will have a negative charge 1+ 1-

What happens when an atom of sodium is put next to an atom of fluorine? After sodium gives its valence electron to fluorine, sodium will have a positive charge and fluorine will have a negative charge What happens when a positively charged object is near a negatively charged object? 1+ 1-

What happens when an atom of sodium is put next to an atom of fluorine? What happens when a positive charged object is near a negatively charged object? 1+ 1- Attraction

What happens when an atom of sodium is put next to an atom of fluorine? The attraction between a negatively charged ion and a positively charged ion is called an ionic bond 1+ 1- Ionic bond

What happens when an atom of sodium is put next to an atom of fluorine? The attraction between a negatively charged ion and a positively charged ion is called an ionic bond When two or more ions are bonded together, we refer to them as an ionic compound 1+ 1- Ionic bond

Binary ionic compounds

Binary ionic compounds Ionic compounds comprised of only two elements are called binary ionic compounds

Binary ionic compounds Ionic compounds comprised of only two elements are called binary ionic compounds For today, every example we look at will be a binary ionic compound

Binary ionic compounds Ionic compounds comprised of only two elements are called binary ionic compounds For today, every example we look at will be a binary ionic compound We will learn about other types of ionic compounds later

Ionic compounds What elements are able to form ionic compounds with one another?

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals Negative ion  Anion

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals Negative ion  Anion Elements that tend to ionize positively are found on the right side of the periodic table

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals Negative ion  Anion Elements that tend to ionize positively are found on the right side of the periodic table These elements have almost full valence shells, so they tend to gain electrons to fill their valence shell

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals Negative ion  Anion Elements that tend to ionize positively are found on the right side of the periodic table These elements have almost full valence shells, so they tend to gain electrons to fill their valence shell Elements on the right side of the periodic table are non-metals

Ionic compounds What elements are able to form ionic compounds with one another? In order to form an ionic bond, you need a positive ion and a negative ion Positive ion  Cation Elements that tend to ionize positively are found on the left side of the periodic table These elements have few electrons in their valence shell, so they tend to lose electrons to fill their valence shells Elements on the left side of the periodic table are all metals Negative ion  Anion Elements that tend to ionize positively are found on the right side of the periodic table These elements have almost full valence shells, so they tend to gain electrons to fill their valence shell Elements on the right side of the periodic table are non-metals Ionic bonds form between cations and anions i.e. between metals and non-metals

Examples of ionic compounds

Examples of ionic compounds Sodium and chlorine

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1−

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The electron that sodium wants to give up is accepted by chlorine, resulting in ionization

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound The electron that sodium wants to give up is accepted by chlorine, resulting in ionization

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound This ionic compound is called sodium chloride The electron that sodium wants to give up is accepted by chlorine, resulting in ionization

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound This ionic compound is called sodium chloride The electron that sodium wants to give up is accepted by chlorine, resulting in ionization Cation is always written first

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound This ionic compound is called sodium chloride The electron that sodium wants to give up is accepted by chlorine, resulting in ionization Cation is always written first Anion is always written second

Examples of ionic compounds Sodium and chlorine Sodium has one valence electron  𝑁𝑎 1+ Chlorine has seven valence electrons  𝐶𝑙 1− The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound This ionic compound is called sodium chloride The electron that sodium wants to give up is accepted by chlorine, resulting in ionization The end of the anion is changed to ‘ide’ to indicate that it is a compound Cation is always written first Anion is always written second

Rules for naming binary ionic compounds

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements Potassium and fluorine Calcium and oxygen Nitrogen and beryllium Phosphorous and lithium

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements Potassium and fluorine potassium fluoride Calcium and oxygen Nitrogen and beryllium Phosphorous and lithium

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements Potassium and fluorine potassium fluoride Calcium and oxygen calcium oxide Nitrogen and beryllium Phosphorous and lithium

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements Potassium and fluorine potassium fluoride Calcium and oxygen calcium oxide Nitrogen and beryllium beryllium nitride Phosphorous and lithium

Rules for naming binary ionic compounds The cation (positively charged ion) must always be written first The anion (negatively charged ion) must always be written second The end of the anion’s name must be changed to ‘ide’ to indicate it is a compound Example: name the binary ionic compound formed between the following elements Potassium and fluorine potassium fluoride Calcium and oxygen calcium oxide Nitrogen and beryllium beryllium nitride Phosphorous and lithium lithium phosphide

Examples of ionic compounds Magnesium and fluorine

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1−

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− Fluorine can only accept one of magnesium’s electrons

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− Fluorine can only accept one of magnesium’s electrons, where does the other go?

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− Fluorine can only accept one of magnesium’s electrons, where does the other go? We need a second fluorine

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound 1- 2+ 1-

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound This ionic compound is called magnesium fluoride 1- 2+ 1-

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound This ionic compound is called magnesium fluoride The chemical formula of magnesium fluoride is: MgF2 1- 2+ 1-

Examples of ionic compounds Magnesium and fluorine Magnesium has two valence electrons  𝑀𝑔 2+ Fluorine has seven valence electrons  𝐹 1− The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound This ionic compound is called magnesium fluoride The chemical formula of magnesium fluoride is: MgF2 1- The subscript indicates how many atoms there are. If no number is written, it implies there is just one 2+ 1-

Rules for writing the chemical formula of ionic compounds

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Calcium bromide Lithium nitride

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  Calcium bromide Lithium nitride

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  NaBr Calcium bromide Lithium nitride

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  NaBr Calcium bromide Ca2+ Br1-  Lithium nitride

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  NaBr Calcium bromide Ca2+ Br1-  CaBr2 Lithium nitride

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  NaBr Calcium bromide Ca2+ Br1-  CaBr2 Lithium nitride Li1+ N3- 

Rules for writing the chemical formula of ionic compounds The symbol for the cation is always written first The symbol for the anion is always written second The subscript numbers indicate how many of each atom there are. No number implies one Example: write the chemical formula for the following ionic compounds Sodium bromide Na1+ Br1-  NaBr Calcium bromide Ca2+ Br1-  CaBr2 Lithium nitride Li1+ N3-  Li3N

Examples of ionic compounds Calcium and nitrogen

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3-

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from?

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from? We need another atom of calcium.

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from? We need another atom of calcium. However, two calciums have one more electron than one nitrogen can accept. Where does this electron go?

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from? We need another atom of calcium. However, two calciums have one more electron than one nitrogen can accept. Where does this electron go? We need another atom of nitrogen.

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from? We need another atom of calcium. However, two calciums have one more electron than one nitrogen can accept. Where does this electron go? We need another atom of nitrogen. However, two atoms of nitrogen need two more electrons than two atoms of calcium can give up. Where do these electrons come from?

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Nitrogen needs one more electron than calcium can give up. Where does this electron come from? We need another atom of calcium. However, two calciums have one more electron than one nitrogen can accept. Where does this electron go? We need another atom of nitrogen. However, two atoms of nitrogen need two more electrons than two atoms of calcium can give up. Where do these electrons come from? We need another atom of calcium

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons Two atoms of nitrogen can accept 6 electrons

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons Two atoms of nitrogen can accept 6 electrons 3(2+) + 2(3-) = 0

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons Two atoms of nitrogen can accept 6 electrons 3(2+) + 2(3-) = 0 Ionic compounds will always be neutral, meaning you must balance the electrons being donated with the electrons being accepted

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons Two atoms of nitrogen can accept 6 electrons 3(2+) + 2(3-) = 0 Ionic compounds will always be neutral, meaning you must balance the electrons being donated with the electrons being accepted Calcium and nitrogen will bond to form calcium nitride  Ca3N2

Examples of ionic compounds Calcium and nitrogen Calcium has two valence electrons  Ca2+ Nitrogen has five valence electrons  N3- Three atoms of calcium can give up 6 electrons Two atoms of nitrogen can accept 6 electrons 3(2+) + 2(3-) = 0 Ionic compounds will always be neutral, meaning you must balance the electrons being donated with the electrons being accepted Calcium and nitrogen will bond to form calcium nitride  Ca3N2 Is there an easier way?

Cross and drop

Cross and drop Ca2+ N3-

Cross and drop Ca2+ N3- Ca3N2

Cross and drop Ca2+ N3- Ca3N2

Cross and drop Ca2+ N3- Ca3N2

Cross and drop Ca2+ N3- Ca3N2 Will this method always work?

Cross and drop Ca2+ N3- Ca3N2 Will this method always work? Yes, but you may have to reduce Ti4+ O2-  Ti2O4  TiO2

Summarizing video https://www.youtube.com/watch?v=zpaHPXVR8WU

Properties of ionic compounds Ionic compounds tend to form lattice structures

Properties of ionic compounds Ionic compounds tend to form lattice structures Ionic compounds dissolve in water Water molecules have a slight charge which pulls the anions and cations apart

Properties of ionic compounds Ionic compounds tend to form lattice structures Ionic compounds dissolve in water When dissolved, ionic compounds are good conductors

Properties of ionic compounds Ionic compounds tend to form lattice structures Ionic compounds dissolve in water When dissolved, ionic compounds are good conductors Recall that electricity is the movement of charged particles

Properties of ionic compounds Ionic compounds tend to form lattice structures Ionic compounds dissolve in water When dissolved, ionic compounds are good conductors Recall that electricity is the movement of charged particles Ions themselves are charged particles