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Simple molecular substances consist of molecules in which the atoms are joined by strong covalent bonds. ... Giant covalent structures contain many atoms joined together by covalent bonds to form agiant lattice. They have high melting and boiling points.

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Properties of simple molecular substances. Low melting and boiling points - This is because the weak intermolecular forces break down easily. Non-conductive - Substances with a simple molecular structure do not conduct electricity. This is because they do not have any free electrons or an overall electric charge.

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An ionic bond is formed from the transfer of electrons from the outer shell of an atom. The atom giving the electron becomes positively charged due to having more protons than electrons. The atom receiving the electrons becomes negatively charged due to having more electrons than protons. The formation of the positive and negatively charged ions forms an ionic bond as of the attraction between the charge of the ions.

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Graphite is one of the more well known forms of carbon as well one of the oldest but unlike diamond, graphite is a conductor and can be used, for instance, as the material in the electrodes of an electrical arc lamp.

The pi orbital electrons de-localized across across the hexagonal atomic sheets of carbon contribute the graphite's conductivity.

Physical characteristics

color is black silver

crystal system is hexagonal

when it fractures its pieces break into flakes

Other characteristics: thin flakes are flexible but inelastic, mineral can leave black marks on hands and paper, conducts electricity. In graphite the effect super lubricity also takes place.

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A covalent Compound is made when two or more nonmetal atoms bond by sharing valence electrons. A shared valence electrons between two different nonmetal atoms are called covalent bonds. Covalent Bonds are formed when two atoms begin sharing electrons. The electrons are attracted to the positively charged nuclei of atoms.

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based on structure, simple covalent substances are made of molecules, are bonded by a pair of electrons they share, which forms a strong covalent bond.

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These are different forms of carbon and this is how their structures look like...

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Structure- they are all linked together strongly. There are a lot of silicon and oxygen atoms that are strongly bonded. There is no set number of atoms joined together in this structure.

Chemical properties- it is not very reactive because it is nonpolar. Used as an insulator and semiconductor.

Physical Properties- it is transparent to gray. It is odorless and it is a crystalline. Melting point is 1600ºC and boiling point is 2230ºC.

Reactivity- it does not react with water or acids. It neutralizes basic metal bases. The solubility depends on the crystalline.

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Examples of ionic compounds include:

1. Table salt—which is NaCl (sodium (metal) and chlorine (non-metal) to form sodium chloride).
2. AgI (silver (metal) iodide (non-metal).

Let’s take a look at the former—table salt.

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Giant covalent structures contain a lot of non-metal atoms, each joined to adjacent atoms by covalent bonds. The atoms are usually arranged into giant regular lattices - extremely strong structures because of the many bonds involved.

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Giant covalent bonding makes the element/compound stronger because of the bonds hold them together. This explains why they are so durable and have high melting points because the bonds are keping them from becoming liquids

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An ionic bond is the bonding between a non-metal and a metal, that occurs when charged atoms (ions) attract.  When this happens, the metal becomes a positive action, and the non-metal becomes a negative anion. This occurs, for example, when sodium and chlorine join to form the common salt, NaCl. This happens after a metal atom loses one or more of its electrons to the nonmetal atom. This makes the bond stronger and harder to break.

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NaBr- Sodium Bromide
KBr- Potassium Bromide
NaCl- Sodium Chloride
NaF- Sodium Fluoride
KI- Potassium Iodine
KCl- Potassium Chloride
CaCl₂-Calcium Chloride
K₂O- Potassium Oxide
MgO- Magnesium Oxide

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The ionic bonds balance the attraction force between positive and negative ions and the repulsion force between similar negative charges in the electron clouds.

These bonds are formed when a metal reacts with a non-metal. Positive ions are formed by metals and negative ions are formed by non-metals.

These compounds remain in the solid state at room temperature and they have high solubility in water.

Atoms with a net negative charge are known as Anion and atoms with a net positive charge are known as Cations.

Ionic compounds have high boiling and melting points because it is quite difficult to break ionic bonds.

These compounds can be produced from their constituent ions by evaporating, precipitation or freezing.

The reaction between metals and non-metals are known as an ionic reaction as they produce ionic compounds.

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when atoms share electrons instead of taking it form the other.they have to be non-metal and metal.

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A simple covalent Bond...

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Silcon dioxide (often called silica) is the main compound found in sand. It is an example of a substance with a giant covalent structure. It contains many silicon and oxygen atoms. All the atoms in its structure are linked to each other by strong covalent bonds. The atoms are joined to each other in a regular arrangement, forming a giant covalent structure. There is no set number of atoms joined together in this type of structure.

Silica has a giant covalent structure containing silicon atoms (grey) and oxygen atoms (red)

Covalent bonding leads to the formation of substances with different types of structures, for example:

small molecules, which contain a fixed number of atoms joined by covalent bonds

giant covalent substances, which contain many atoms joined by covalent bonds

High melting points and boiling points

Substances with giant covalent structures are solids at room temperature. They have very high melting points and boiling points. This is because large amounts of energy are needed to overcome their strong covalent bonds to make them melt or boil.

Conduction of electricity

Most substances with giant covalent structures have no charged particles that are free to move. This means that most cannot conduct electricity. Graphite, a form of carbon which can conduct electricity, is an exception.

The boiling point of silicone dioxide is at 2,230°C, and since Silicon dioxide is very hard. It has a very high melting point (1,610 °C) and boiling point (2,230 °C), is insoluble in water, and does not conduct electricity. All of giant covalent structures have these similar properties.

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All ionic compounds form crystal structures

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An ionic compound is a giant structure of ions. The ions have a regular, repeating arrangement called an ionic lattice. The lattice is formed because the ions attract each other and form a regular pattern with oppositely charged ions next to each other.

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Structure- it is a giant ionic structure, it has an endless lattice of ions. They are arranged in such a way that they form crystal lattice.

Chemical properties- when it reacts it reacts quickly, and it is exothermic. The reaction of it with acids is double displacement.

Physical properties- it does not have an odor, white, cubic crystals and it has a salty taste. The melting point is 800.8°C and the boiling point is 1465°C, it is soluble in water.

Reactivity- it does not conduct electricity in its solid state. The melting and boiling point are high because the atoms are strongly bonded together. They are good conductors of heat and electricity in liquid states.

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Diamonds are an example of  Giant Covalent Bonds.
along with Graphite.

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Covalent Bonds are when two non-metal atoms are sharing electrons with each other. Carbon Dioxide is a chemical compound which is a gas at room temperature. At a molecular level it is made up of two carbon atoms and one oxygen atom. People and animals realize carbon dioxide when they breathe out. The gas is odorless and is a colorless gas. It has sufficiently high concentration is pretty dense. Carbon Dioxide reacts with alkalis to make carbonates and bicarbonates. It is an acidic oxide and reacts with water to give carbonic acid.

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Giant covalent bonding is when simple covalent bonding forms a lot of bonds making very strong structures because of all the bonds that are holding them together. These form things like diamond and carbon. The results of covalent bonding always have high melting points because the bonds make it easier for them to stay together.

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Ionic compounds are formed by ions. An example of an ionic compound is Lithium Fluorideb, which is formed from ionic bonding. The formula for it is LiF.

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•Structure - There could be billions or trillions of chloride ions and sodium ions in the structure, which makes it a giant ionic compound. It is an endlessly repeating lattice of ions.

•Properties: -

•It is a colorless and odorless powder or substance that tastes salty.

•Sodium Chloride has a very high melting point of 801 °C, and a high boiling point of 1,413 °C, because the electrostatic attraction between the positive and negative ions is very high, and therefore, it takes a lot of heat energy to melt or boil them.

•Sodium Chloride is a very brittle substance because the electrons are tightly held together by the ions, which cannot move relative to each other.

•Sodium chloride doesn’t conduct electricity because there are no electrons that are free to move around.

•The compound is soluble in water, but insoluble in organic solvents like methanol.

•The molecular weight of Sodium Chloride is 58.44 g/mol.

•2Na+Cl2=2NaCl

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•Structure - Covalent substances are made up of molecules, that are bound together by shared electrons.

•Properties: -

•The force between the molecule is low and therefore, causes low melting and boiling points. The melting point of Carbon Monoxide is -205 °C, whereas the boiling point is -191.5 °C.

•Carbon Monoxide does not conduct electricity because it is a non-metal and the molecules overall don’t have an electric charge.

•It is a colorless, odorless, tasteless and poisonous gas that causes nervous system problems when inhaled.

•The atomic weight of Carbon Monoxide is 28.01 g/mol.

•Carbon Monoxide is an extremely flammable gas and when exposed to fire, it could even explode.

•Carbon monoxide can react with nitrogen monoxide to create carbon dioxide.

•2CO+O2 = 2CO2.

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Ionic bonding is observed because metals have few electrons in their outer-most orbitals. By losing those electrons, these metals can achieve noble gas configuration and satisfy the octet rule. Similarly, nonmetals that have close to 8 electrons in their valence shells tend to readily accept electrons to achieve noble gas configuration. In ionic bonding, more than 1 electron can be donated or received to satisfy the octet rule. The charges on the anion and cation correspond to the number of electrons donated or received. In ionic bonds, the net charge of the compound must be zero

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Lithium fluoride is an inorganic compound with the chemical formula LiF. It is a colorless solid, that transitions to white with decreasing crystal size. Although odorless, lithium fluoride has a bitter-saline taste. Its structure is analogous to that of sodium chloride, but it is much less soluble in water.Formula: LiFMolar mass: 25.939 g/molBoiling point: 1,676 °CDensity: 2.64 g/cm³Appearance: white powder or transparent crystals, hygroscopicChemSpider ID: 23007PubChem CID: 224478

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Lithium fluoride is an inorganic compound with the chemical formula LiF. It is a colorless solid, that transitions to white with decreasing crystal size. Although odorless, lithium fluoride has a bitter-saline taste. Its structure is analogous to that of sodium chloride, but it is much less soluble in water.Formula: LiFMolar mass: 25.939 g/molBoiling point: 1,676 °CDensity: 2.64 g/cm³Appearance: white powder or transparent crystals, hygroscopicChemSpider ID: 23007PubChem CID: 224478

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ionic compounds are made up of ions and covalent compounds are made when two or more nonmetal atoms bond by sharing valence electrons.

valence: relating to or denoting electrons involved in or available for chemical bond formation.

whats the difference?

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Giant Covalent Bonding Structure of a Diamond

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Properties of ionic compounds-
Ionic compounds have high boiling and melting points because they are strong and require a lot of energy to break. 
Ionic compounds form crystals.
These are compounds are brittle and break into very small little pieces.
They do not conduct electricity in a solid state but they do conduct electricity in their molten state. 
The electrostatic forces of attractions between oppositely charged ions lead to the formation of ions. 
Electrovalent compounds mostly dissolve in water and are insoluble in solvents like oil, petrol, etc. 

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Reactions:Reaction of carbon with water. Carbon, either as graphite or diamond does notreact with water under normal conditions. Under more forsing conditions, thereaction becomes important. In industry, water is blown through hot coke.

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Reactions:Reaction of carbon with water. Carbon, either as graphite or diamond does notreact with water under normal conditions. Under more forsing conditions, thereaction becomes important. In industry, water is blown through hot coke.

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MgSO4

Magnesium Sulphate is an example of an ionic compound. Commonly known as epsom salt.

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Bonding : Graphite has a giant covalent structure consisting of layers of carbon atoms. Carbon atoms have 4 valence electrons that are available for bonding. In graphite, each carbon atom is covalently bonded to 3 other carbon atoms. Therefore, every carbon atom has 1 electron that is not used for bonding.

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Bonding : Graphite has a giant covalent structure consisting of layers of carbon atoms. Carbon atoms have 4 valence electrons that are available for bonding. In graphite, each carbon atom is covalently bonded to 3 other carbon atoms. Therefore, every carbon atom has 1 electron that is not used for bonding.

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A covalent bond is formed when a pair of electrons is shared between two atoms. These shared electrons are found in the outer shells of the atoms. In general, each atom contributes one electron to the shared pair of electrons. Non Metal-Non Metal

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Reactions:  The bonds that form the methane molecule are covalent bonds with a tetrahedral geometry. ... Combustion reactions with methane produce carbon dioxide, water, heat, and in the case of incomplete combustion, carbon monoxide. Halogenationreactions occur when a halogen reacts withmethane to form a methyl halide.

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Reactions:  The bonds that form the methane molecule are covalent bonds with a tetrahedral geometry. ... Combustion reactions with methane produce carbon dioxide, water, heat, and in the case of incomplete combustion, carbon monoxide. Halogenationreactions occur when a halogen reacts withmethane to form a methyl halide.

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Properties- Very high melting points
Substances with giant covalent structures have very high melting points, because a lot of strong covalent bonds must be broken. Graphite, for example, has a melting point of more than 3,600ºC.
Conductivity does not conduct electricity.

Bonding-  A covalent bond is formed when a pair of electrons is shared between two atoms. These shared electrons are found in the outer shells of the atoms. In general, each atom contributes one electron to the shared pair of electrons. Non Metal-Non Metal

Facts-  Each carbon atom uses three of its electrons to form simple bonds to its three close neighbour. That leaves a fourth electron in the bonding level. These "spare" electrons in each carbon atom become delocalised over the whole of the sheet of atoms in one layer. They are no longer associated directly with any particular atom or pair of atoms, but are free to wander throughout the whole sheet.

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A covalent bond forms when the electrons on the other shells of two non-metals are shared. These bonds tend to be very strong and need lots of energy to be broken apart. These bond also are mostly found in molecules with low boiling and melting points. This is because there is an even number of electrons in the outer shell, as the electron charge around each atom is even.

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Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion. Ionic bonds require an electron donor, often a metal, and an electron acceptor, a nonmetal.

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Structure- the carbon is in the middle and the two oxygen molecules by its sides.

Chemical properties- it is non-polar and it is very stable and it does not react.

Physical properties- it is a colorless gas. The boiling point is about -78.4°C, the melting point is -56.61°C.

Reactivity- it is an acidic oxide. The melting and boiling point is very low because the atoms are further apart.

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Covalent Bonding-

Properties- -Low melting points and boiling points.
-Low enthalpies of fusion and vaporization These properties are usually one or two orders of magnitude smaller than they are for ionic compounds.
-Soft or brittle solid forms.
-Poor electrical and thermal conductivity.

Bonding- A covalent bond is formed when a pair of electrons is shared between two atoms. These shared electrons are found in the outer shells of the atoms. In general, each atom contributes one electron to the shared pair of electrons. Non Metal-Non Metal

Reaction-  Covalency is greatest between atoms of similar electronegativities. Thus, covalent bonding does not necessarily require that the two atoms be of the same elements, only that they be of comparable electronegativity. Covalent bonding that entails sharing of electrons over more than two atoms is said to be delocalized.

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Methane is lighter than air, having a specific gravity of 0.554. It is only slightly soluble in water. It burns readily in air, forming carbon dioxide and water vapour; the flame is pale, slightly luminous, and very hot. The boiling point of methane is −162 °C (−259.6 °F) and the melting point is −182.5 °C (−296.5 °F). Methane in general is very stable, but mixtures of methane and air, with the methane content between 5 and 14 percent by volume, are explosive. Explosions of such mixtures have been frequent in coal mines and collieries and have been the cause of many mine disasters.

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Methane is lighter than air, having a specific gravity of 0.554. It is only slightly soluble in water. It burns readily in air, forming carbon dioxide and water vapour; the flame is pale, slightly luminous, and very hot. The boiling point of methane is −162 °C (−259.6 °F) and the melting point is −182.5 °C (−296.5 °F). Methane in general is very stable, but mixtures of methane and air, with the methane content between 5 and 14 percent by volume, are explosive. Explosions of such mixtures have been frequent in coal mines and collieries and have been the cause of many mine disasters.

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Giant covalent bonds contain many covalent bonds in a fixed lattice structure. Between each atom of carbon in a diamond, there are 4 strong covalent bonds.

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An ionic bond is when a metal gives away an electron(s) to a non-metal, so that both outer shells are full and stable. This leads to an electric charge due to the loss or gain of an electron. Therefore, they attract each other and form a bond

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Ionic compounds/bonding, Covalent ( simple & giant) compounds/bonding 

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Ionic compounds/bonding, Covalent ( simple & giant) compounds/bonding 

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Ionic bonding:
Ionic bonding is the bonding between two atoms where an atom loses an electron and gives it to an atom that has 7 electrons so that it may fill its shell, while the atom that loses an electron has 1 in its outer shell and gets rid of it so that it empties its outer shell.The atom that loses its electron becomes positive while the atom that gains an electron becomes negative.This happens through electrostatic attraction.An atom may gain/lose 1 or more  electrons according to the amount it has. It Ionic binding only occurs between a metal and a non-metal.

Ionic Compounds:
Ionic compounds is a group of ions that are stuck together by electrostatic forces through ionic bonding. These have positively charged ions which are called cations and negatively charged ions called anions.

Simple covalent bonding:
When atoms bond by sharing electrons. One pair of shared electrons is a single covalent bond. Two shared pairs is a double covalent bond, and three shared pairs is a triple covalent bond.

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Graphite:

Graphite is a naturally-occurring form of crystalline carbon. It is a native element mineral found in metamorphic and igneous rocks.Graphite is a mineral of extremes. It is extremely soft, cleaves with very light pressure, and has a very low specific gravity.

Graphite has a high melting point,soft, slippery feel. It is used to make pencils and as a dry lubricant for things like locks. It also has a lower density than diamond. Graphite does not react with water under normal conditions.

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Structure: CI-

Physical Properties: Color: Greenish-Yellow, Phase: Gas, Smell: suffocating smell, Density: About two and one-half times as dense as air, BP: -34.05°C and MP: -101°C

Chemical Properties: Chemical Formula: CI, Toxicity: Highly Toxic, Compounds: PVC, hydrochloric acid and Sodium chloride (table salt), reactivity with metals: most metals react with Chloride only after being heated up

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Ionic bonding is the complete transfer of valence electron(s) between atoms and is a type of chemicalbond that generates two oppositely charged ions. It is observed because metals with few electrons in its outer-most orbital.

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Compound: sodium Chloride (NaCl)

Structure: sodium chloride is known as a typical ionic compound that consists of an endlessly respecting lattice of ions. It is known as having a giant ionic structure.

Properties physical/chemical: sodium chloride is white cubic crystals with a salty taste, it is completely odorless and has salt that is hygroscopic in nature because of its strong electrostatic force of attraction between the ions. It’s boiling point is 1465 degrees Celsius, and it’s melting point is 800.8 degrees Celsius. The vapour pressure of it is 856 degrees C at 1 mm Hg and it’s density is 2.165g cm3.

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Ionic bonds are the transfer of valence electrons from the atom of one element to another, generating two completely opposite charged electrons, for example magnesium oxide (MgO), or Lithium Fluoride (LiF). The compound I chose for this type of chemical bonding is sodium chloride (NaCl). Sodium Chloride also known as salt is an essential compound needed for the human body it is used to absorb nutrients and maintain blood pressure. It has a 1:1 ration in the compound and is soluble in water, ammonia, methanol, formic acid, Form-amide. Sodium Chloride is formed as tiny white crystals and is odorless but has a characteristic taste, it is made up of equal numbers of sodium and chloride ions. It has a melting point of 800 degrees Celsius, and a boiling point of 1465 degrees Celsius. It has a strong electrostatic force between them. It is readily soluble in water and other polar solvents.

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Ionic Bonding
Properties-  Ionic Compounds have high boiling and melting points as they’re very strong and require a lot of energy to break.
The electrostatic forces of attraction between oppositely charged ions lead to the formation of ions.
Ionic compounds form crystals.
These compounds are brittle and break into small pieces easily.
Electrovalent compounds usually dissolve in water and are insoluble in solvents like oil, petrol, kerosene, etc.
Ionic compounds do not conduct electricity in a solid state but they do conduct electricity in the molten state.
In comparison to molecular compounds, ionic compounds have higher enthalpies of fusion and vaporization.

Bonding- The Plus And Negative Are Closely Bonded Sharing Electrons Together. Ionic Bonding Takes Place Between Non Metal And Metal.

Reaction-  Ionic bonding can result from a redox reaction when atoms of an element (usually metal), whose ionization energy is low, give some of their electrons to achieve a stable electron configuration. However, the ions themselves can be complex and form molecular ions.

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Ionic compounds are made out of ions rather than molecules. Instead of sharing electron in covalent bonds, ionic compound atoms are transferring electrons from one atom to another atom to try to form an ionic bond that relies on electrostatic attraction to keep the atom together. Covalent bonds that are bonded with molecules share electrons and act as a stable, single entity while an ionic bond results in independent ions that have a positive or negative charge, because most of their special structure, ionic compounds have a unique property and reacts easily with other ionic compounds when placed in different solutions.

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Ionic bonding
Ionic bonding is the complete transfer of valence electron between atoms and is a type of chemical bond that generates two oppositely charged ions. It is observed because metals with few electrons in its outer-most orbital.

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There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 - 200 kcal/mol). Whether two atoms can form a covalent bond depends upon their electronegativity for example the power of an atom in a molecule to attract electrons to itself. If two atoms differ considerably in their electronegativity  as sodium and chloride do then one of the atoms will lose its electron to the other atom. This results in a positively charged ion and negatively charged ion. The bond between these two ions is called an ionic bond.

Ions occur between:

Two non-metals

Covalent occur between:

One metal and one non-metal

Boiling point for Ionic Bonding:

Low

Boiling point for Covalent Bonding:

High

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Positive and negative ions are formed when a metal reacts with a non-metal, this is completed by the process of transferring electrons. The oppositely charged electrons are extremely attracted to each other which forms ionic bonds.  The example shown is an ionic bond between Lithium and Chlorine.

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Simple covalent bonding is when an atom shares its electrons with another atom. Unlike the ionic bonding this type of bonding actually shares its electrons with the atom rather than giving it away. This process only takes place between 2 nonmetals which need to be stabilized

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Before we actually get into what exactly ionic compounds are, let’s see what an ion is!

Well, in theory, an ion is an atom or molecule, that has either gained or lost [one—or more of] their valence electrons to another element (often the non-metal giving the electron to a metal)—in order to form an ionic bond [as the name may suggest].

In turn, this gives the giving atoms (or molecules) a positive net electric charge (AKA a cation), whilst he receiver of the electrons(s) gets a negative electronic charge (AKA anion)

And together, when these opposing ions give, or take electrons, then bond—via electrostatic forces [ie. forces between particles that are caused by their electric charges]. This is what we call an ionic bond.

As for an ionic compound...well, it’s pretty obvious. An ionic compound is a composition of two [or more] separate elements, [ionically].

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If atoms have similar electronegativity’s (the same affinity for electrons), covalent bonds are most likely to occur. Because both atoms have the same affinity for electrons and neither has a tendency to donate them, they share electrons in order to achieve octet configuration and become more stable.