When an element shares electrons with other atoms of the same or different elements to acquire stable electronic configuration

it is called covalency.

If an atom shares 1 electron, its covalency is equal to 1

If it can share 2 electrons, its covalency is 2.

When an element shares electrons with other atoms of the same or different elements to acquire stable electronic configuration

it is called covalency.

If an atom shares 1 electron, its covalency is equal to 1

If it can share 2 electrons, its covalency is 2.

When an element shares electrons with other atoms of the same or different elements to acquire stable electronic configuration

it is called covalency.

If an atom shares 1 electron, its covalency is equal to 1

If it can share 2 electrons, its covalency is 2.

The bonds that hold atoms together in compounds are called intramolecular forces.

The 3 main types of intramolecular forces are ionic bonds, covalent bonds, and metallic bonds.

This video will focus on covalent bonds: Ionic bonds and Metallic bonds will be featured

in their own videos.

Covalent bonds are stable because the bonding atoms achieve noble gas configuration by sharing

electrons.

The name, covalent, should suggest to you that the atoms are sharing their valence electrons.

We can show this with a Lewis dot diagram..

The 3 main types of intramolecular forces are ionic bonds, covalent bonds, and metallic bonds.

This video will focus on covalent bonds: Ionic bonds and Metallic bonds will be featured

in their own videos.

Covalent bonds are stable because the bonding atoms achieve noble gas configuration by sharing

electrons.

The name, covalent, should suggest to you that the atoms are sharing their valence electrons.

We can show this with a Lewis dot diagram..

Hydrogen fluoride (HF) is a molecule with a single covalent bond formed between two

atoms.

This video will focus on covalent bonds: Ionic bonds and Metallic bonds will be featured

in their own videos.

Covalent bonds are stable because the bonding atoms achieve noble gas configuration by sharing

electrons.

The name, covalent, should suggest to you that the atoms are sharing their valence electrons.

We can show this with a Lewis dot diagram..

Hydrogen fluoride (HF) is a molecule with a single covalent bond formed between two

atoms.

Fluorine has 7 valence electrons, and hydrogen has one.

Covalent bonds are stable because the bonding atoms achieve noble gas configuration by sharing

electrons.

The name, covalent, should suggest to you that the atoms are sharing their valence electrons.

We can show this with a Lewis dot diagram..

Hydrogen fluoride (HF) is a molecule with a single covalent bond formed between two

atoms.

Fluorine has 7 valence electrons, and hydrogen has one.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

The name, covalent, should suggest to you that the atoms are sharing their valence electrons.

We can show this with a Lewis dot diagram..

Hydrogen fluoride (HF) is a molecule with a single covalent bond formed between two

atoms.

Fluorine has 7 valence electrons, and hydrogen has one.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Hydrogen fluoride (HF) is a molecule with a single covalent bond formed between two

atoms.

Fluorine has 7 valence electrons, and hydrogen has one.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

Fluorine has 7 valence electrons, and hydrogen has one.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

We can see an example of that in carbon dioxide, CO2.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

We can see an example of that in carbon dioxide, CO2.

By sharing 2 electrons in a bond, now hydrogen has 2 valence electrons, and has the same

electron configuration as the noble gas helium.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

We can see an example of that in carbon dioxide, CO2.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Fluorine now has 8 valence electrons, and has the same electron configuration as the

noble gas neon.

We can replace those 2 shared electrons in the diagram by a single line, representing

the single covalent bond.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

We can see an example of that in carbon dioxide, CO2.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

Sometimes, two atoms share more than 2 electrons, in the case of a double or triple covalent

bond.

We can see an example of that in carbon dioxide, CO2.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can see an example of that in carbon dioxide, CO2.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can see an example of that in carbon dioxide, CO2.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

The Lewis dot structure looks like this: Carbon has 4 valence electrons, and Oxygen has 6

valence electrons.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

Carbon needs 4 more electrons to achieve noble gas configuration.

Oxygen needs 2 more electrons to achieve noble gas configuration.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

The bond between these identical atoms is called a non-polar covalent bond.

Hydrogen, for instance, exists in nature as a diatomic molecule, H2.

This can be achieved if the carbon atom forms 2 double bonds with each oxygen atom.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

The bond between these identical atoms is called a non-polar covalent bond.

Hydrogen, for instance, exists in nature as a diatomic molecule, H2.

The two hydrogen atoms pull equally on the shared pair of electrons in the bond, so there

is no directionality, or POLARITY, of the bond.

We can replace the two shared pairs of electrons in the diagram with 2 straight lines, representing

a double bond.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

The bond between these identical atoms is called a non-polar covalent bond.

Hydrogen, for instance, exists in nature as a diatomic molecule, H2.

The two hydrogen atoms pull equally on the shared pair of electrons in the bond, so there

is no directionality, or POLARITY, of the bond.

Compare that with the bonds in a polar molecule, like water, H2O.

If the two atoms in a covalent bond are identical, they have the exact same electronegativity

as each other.

The bond between these identical atoms is called a non-polar covalent bond.

Hydrogen, for instance, exists in nature as a diatomic molecule, H2.

The two hydrogen atoms pull equally on the shared pair of electrons in the bond, so there

is no directionality, or POLARITY, of the bond.

Compare that with the bonds in a polar molecule, like water, H2O.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

The bond between these identical atoms is called a non-polar covalent bond.

Hydrogen, for instance, exists in nature as a diatomic molecule, H2.

The two hydrogen atoms pull equally on the shared pair of electrons in the bond, so there

is no directionality, or POLARITY, of the bond.

Compare that with the bonds in a polar molecule, like water, H2O.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

The two hydrogen atoms pull equally on the shared pair of electrons in the bond, so there

is no directionality, or POLARITY, of the bond.

Compare that with the bonds in a polar molecule, like water, H2O.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

Compare that with the bonds in a polar molecule, like water, H2O.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

Compare that with the bonds in a polar molecule, like water, H2O.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

Oxygen is much more electronegative than hydrogen, so the electrons in the covalent bonds spend

more time around the oxygen than around the hydrogen.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

We call this kind of uneven sharing of electrons a polar covalent bond.

We call this kind of uneven sharing of electrons a polar covalent bond.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

Notice that this results in the water molecule being polar as a whole - one side of the molecule

is more negative than the other side.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

That’s a result of the polar covalent bonds that hold the water molecule together.

A lowercase delta is used to show the partial negative charge on the oxygen atom and the

partial positive charge on the hydrogen atoms.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

That’s a result of the polar covalent bonds that hold the water molecule together.

But consider the carbon tetrachloride molecule, CCl4.

We use this delta notation to distinguish these partial charges from the full charges

carried by ions.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

That’s a result of the polar covalent bonds that hold the water molecule together.

But consider the carbon tetrachloride molecule, CCl4.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might get confused between molecules which contain polar covalent bonds and molecules

which are polar as a whole.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

That’s a result of the polar covalent bonds that hold the water molecule together.

But consider the carbon tetrachloride molecule, CCl4.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

Water is both - it contains polar bonds, and is a polar molecule (as a whole) because one end of the molecule is slightly positive and the other side is slightly negative.

That’s a result of the polar covalent bonds that hold the water molecule together.

But consider the carbon tetrachloride molecule, CCl4.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point

That’s a result of the polar covalent bonds that hold the water molecule together.

But consider the carbon tetrachloride molecule, CCl4.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point in 4 opposite directions,

so they cancel each other out.

But consider the carbon tetrachloride molecule, CCl4.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point in 4 opposite directions,

so they cancel each other out.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chlorine is more electronegative than carbon, so this molecule has 4 polar covalent bonds.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point in 4 opposite directions,

so they cancel each other out.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point in 4 opposite directions,

so they cancel each other out.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

You might think, adding the 4 bonds together, this molecule is going to be VERY polar as

a result.

But actually, when you look at the 3 dimensional structure, you see that the 4 bonds point in 4 opposite directions,

so they cancel each other out.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

so they cancel each other out.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

And if the electronegativities differ by more than 1.7, it’s an ionic bond.

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

Are covalent bonds, like many ionic bonds, disrupted by water?

You can’t find one SIDE of CCl4 that is more negative or positive than the other,

so carbon tetrachloride as a whole is a nonpolar molecule.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

Are covalent bonds, like many ionic bonds, disrupted by water?

Some are, some are not.

Chemists generally measure the polarity of a bond according to a scale established by

Linus Pauling {show table of values}.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

Are covalent bonds, like many ionic bonds, disrupted by water?

Some are, some are not.

For instance, Sucrose, C12H22O11 (that’s table sugar), is a molecule with atoms held

together by covalent bonds.

If the relative electronegativities of the two bonded atoms differ by less than 0.4 on

the Pauling scale, the bond is considered nonpolar covalent.

If the difference in relative electronegativities is between 0.4 and 1.7, we call it a polar

covalent bond.

Are covalent bonds, like many ionic bonds, disrupted by water?

Some are, some are not.

For instance, Sucrose, C12H22O11 (that’s table sugar), is a molecule with atoms held

together by covalent bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Are covalent bonds, like many ionic bonds, disrupted by water?

Some are, some are not.

For instance, Sucrose, C12H22O11 (that’s table sugar), is a molecule with atoms held

together by covalent bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

Some are, some are not.

For instance, Sucrose, C12H22O11 (that’s table sugar), is a molecule with atoms held

together by covalent bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

For instance, Sucrose, C12H22O11 (that’s table sugar), is a molecule with atoms held

together by covalent bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

Even though some covalent bonds can come apart in water, they are considered strong bonds,

as are ionic bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

Even though some covalent bonds can come apart in water, they are considered strong bonds,

as are ionic bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

Even though some covalent bonds can come apart in water, they are considered strong bonds,

as are ionic bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

Even though some covalent bonds can come apart in water, they are considered strong bonds,

as are ionic bonds.

If you put sucrose, or other sugars in water, the covalent bonds stay intact and a sugar-water

solution does not conduct electricity as well as a salt-water solution.

Acids, on the other hand, like HCl, hydrochloric acid, are covalent compounds which readily

dissociate into H+ and Cl- ions, so they DO conduct electricity.

We call these substances that ionize when they dissolve “electrolytes.”

Most soluble salts, acids, and bases act this way.

Even though some covalent bonds can come apart in water, they are considered strong bonds,

as are ionic bonds.

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Amphoteric Oxide

Basic Oxide

Neutral Oxide

Acidic Oxide

Add a lit splint and it relights

Add a lit splint and it burns with a pop

Add a glowing splint and it relights

Add a glowing splint and it burns with a pop

Water

Hydrogen peroxide

manganese

manganese (IV) Oxide

Displacment

Decomposition

Precipitation

Synthesis

manganese (IV) oxide

Salt

Sugar

Hydrogen peroxide

True

False

Reacts with acids only

Reacts with bases only

Reacts with acids and bases

Do not react with acids or bases

potassium oxide

iron (II) oxide

aluminum oxide

calcium oxide

sulfurous acid

sulfuric acid

salt

carbon dioxide

water

hydrogen

downward delivery

upward delivery

gas syringe

over water

Reacts with acids only

Reacts with bases only

Reacts with acids and bases

Do not react with acids or bases

Add to water and test with litmus

Add to acid and test with litmus

Test acid with litmus, add base to acid and test with litmus

Add base to acid and test with litmus

O

O₂

O₃

high melting point

hardness

octahedral shape

durability

have octahedral shape

have same density

form carbon(IV) oxide o combustion

conduct electricity

Graphite

Diamond

Lampblack

Soot

producer gas

natural gas

synthetic gas

industrial gas

Carbon(IV) oxide

Carbon(II) oxide

Sulphur (IV) oxide

Sulphur (VI) oxide

wood charcoal

animal charcoal

carbon fibres

carbon black

CH₄ and H₂O

CH₄ and H₂

CO and H₂

CO₂ and H₂

graphite

soot

charcoal

lamp black

hydrogen and trioxocarbonate(IV) acid

hydrogen, oxygen and carbon(II)oxide

hydrogen and carbon(II) oxide

hydrogen and carbon(IV) acid

electrons in both the 2s and 2p orbitals are equivalent

the electrons in all the orbitals of carbon are equivalent

the 2s and 2p orbitals hybridised

all the atomic orbitals of carbon hybridise

acid

base

salt

water

acid

base

salt

non-electrolyte

red

purple

blue

yellow

HBr

KBr

H₂O

KOH

Hydrofluoric acid

Fluorous acid

Fluoric acid

Flourine acid

the concentration of OH- ions

the concentration of salt ions

the concentration of H+ ions

concentration

color

temperature

taste

LiBr

BrLi

NaCl

NaOH

dissolves metals

turns blue litmus red

has a bitter taste

Acids

Bases

Salts

All

Acids

Bases

Salts

All

Acid

Base

Acid

Base

HBr

HB

HBrO₃

HBO₃

HIO₂

HIo

HI

IO₂

H₂CO₃

H₂CrO₄

H₂C₂O₄

HCO₃

Mg(OH)₃

Mg(OH)₂

MgOH

NaOH

Na(OH)₂

Na₂O

Fe(OH)₃

Fe(OH)₂

FeOH

Sn₂OH

Sn(OH)₂

Sn₂OH₂

Sn₃(OH)₂

colourless to milky

burns with pop

relights a glowing splint

the solution goes clear

pH increases

pH decreases

pH remains the same

1

5

11

14

Neutral

Weak base

Base

Strong acid

7

8

3

11

Acid

Neutral

Base

Buffer

0-6.9

7.1-14

0-14

1–7

1–5

0–14

1–20

0

4

7

12

Greater than 7 (>7)

Less than 7 (<7)

Equal to 7 (7)

Between 0–14

Hydrogen

Carbon dioxide

Oxygen

water vapour

Acid

Base

Acid

Base

Acid

Base

Acid

Base

Acid

Base

Metal Hydroxides

Metal Oxides

Metals

Metal Sals

True

False

True

False

True

False

True

False

True

False

True

False

Renewable energy.

Independent energy.

Nonrenewable energy.

Inexhaustible energy.

Coal.

Solar.

Oil.

Fish.

It only has a single-use.

It releases carbon dioxide into the air.

We will never run out of it!

It can grow back!

Fish.

Hydro.

Tidal.

Natural gas.

Nonrenewable.

Renewable.

Inexhaustible.

None of the above.

Chocolate chips.

Died ancient animals.

Died ancient trees.

Old carboniferous rocks.

Oxygen.

Hydrogen.

Water.

Carbon.

Carboniferous period.

Jurassic period.

Triassic period.

Mesozoic era.

Specialized leaves.

Feet.

Wood.

Longer roots.

Russia.

Australia.

Canada.

Italy.

Fertilizer.

Sun.

Water.

Pressure.

Coal mines.

Coal drags.

Coal seams.

Coal stripe.

Mountain top removal.

Underground mining.

Underwater mining.

Open pit mining.

Open pit mining.

Strip mining.

Mountain top removal.

Underground mining.

Mountain top removal.

Strip mining.

Open pit mining.

Underground mining.

Purple lung disease.

Surface environment destruction.

Subsidence.

Acid mine drainage.

Gingivitis disease.

Black lung disease.

Blue lung disease.

None of the above.

Environmental restoration.

Electricity generation.

Steel manufacturing.

Powering cars.

Restore the environment after mining.

Pay miners more money.

Destroy the environment and not fix it.

None of the above.

Mountains and valleys.

Mammals and dinosaurs.

Lakes and rivers.

Coastal swamps.