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how do ionic bonds differ from covalent bonds

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From Wikipedia

Ionic bond

An ionic bond is a type of chemical bond that involves a metal and a nonmetalion (or polyatomic ions such as ammonium) through electrostatic attraction. In short, it is a bond formed by the attraction between two oppositely charged ions.

The metal donates one or more electrons, forming a positively charged ion or cation with a stable electron configuration. These electrons then enter the non metal, causing it to form a negatively charged ion or anion which also has a stable electron configuration. The electrostatic attraction between the oppositely charged ions causes them to come together and form a bond.

For example, common table salt is sodium chloride. When sodium (Na) and chlorine (Cl) are combined, the sodium atoms each lose an electron, forming cations (Na+), and the chlorine atoms each gain an electron to form anions (Cl−). These ions are then attracted to each other in a 1:1 ratio to form sodium chloride (NaCl).

Na + Cl → Na+ + Cl−→ NaCl

The removal of electrons from the atoms is endothermic and causes the ions to have a higher energy. There may also be energy changes associated with breaking of existing bonds or the addition of more than one electron to form anions. However, the attraction of the ions to each other lowers their energy. Ionic bonding will occur only if the overall energy change for the reaction is favourable – when the bonded atoms have a lower energy than the free ones. The larger the resulting energy change the stronger the bond. The low electronegativity of metals and high electronegativity of non-metals means that the energy change of the reaction is most favorable when metals lose electrons and non-metals gain electrons.

Pure ionic bonding is not known to exist. All ionic compounds have a degree of covalent bonding. The larger the difference in electronegativity between two atoms, the more ionic the bond. Ionic compounds conduct electricity when molten or in solution. They generally have a high melting point and tend to be soluble in water.

Ionic structure

Ionic compounds in the solid state form lattice structures. The two principal factors in determining the form of the lattice are the relative charges of the ions and their relative sizes. Some structures are adopted by a number of compounds; for example, the structure of the rock salt sodium chloride is also adopted by many alkali halides, and binary oxides such as MgO.

Strength of an ionic bond

For a solid crystalline ionic compound the enthalpy change in forming the solid from gaseous ions is termed the lattice energy. The experimental value for the lattice energy can be determined using the Born-Haber cycle. It can also be calculated using the Born-Landé equation as the sum of the electrostatic potential energy, calculated by summing interactions between cations and anions, and a short range repulsive potential energy term. The electrostatic potential can be expressed in terms of the inter-ionic separation and a constant (Madelung constant) that takes account of the geometry of the crystal. The Born-Landé equation gives a reasonable fit to the lattice energy of e.g. sodium chloride where the calculated value is −756 kJ/mol which compares to −787 kJ/mol using the Born-Haber cycle.

Polarization effects

Ions in crystal lattices of purely ionic compounds are spherical; however, if the positive ion is small and/or highly charged, it will distort the electron cloud of the negative ion, an effect summarised in Fajans' rules. This polarization of the negative ion leads to a build-up of extra charge density between the two nuclei, i.e., to partial covalency. Larger negative ions are more easily polarized, but the effect is usually only important when positive ions with charges of 3+ (e.g., Al3+) are involved. However, 2+ ions (Be2+) or even 1+ (Li+) show some polarizing power because their sizes are so small (e.g., LiI is ionic but has some covalent bonding present). Note that this is not the ionic polarization effect which refers to displacement of ions in the lattice due to the application of an electric field.

Ionic versus covalent bonds

In an ionic bond, the atoms are bound by attraction of opposite ions, whereas, in a covalent bond, atoms are bound by sharing electrons. In covalent bonding, the molecular geometry around each atom is determined by VSEPR rules, whereas, in ionic materials, the geometry follows maximum packing rules.

In reality, purely ionic bonds do no


From Yahoo Answers

Question:i have to do a short answer pleas help! thanks

Answers:In ionic bonding, the metal DONATES one or more electrons, forming a positively charged ion or cation with a stable electron configuration. on the other hand, a covalent bonding is the stable balance of attractive and repulsive forces between atoms when they SHARE electrons.

Question:How do i tell what type of bond it is?, the 3 options are ionic or covalent, or metallic? Here are few examples (the numbers are suppose to be subscripts but i don't how to make them subscripts so just pretend the numbers are subscripts) CH4 (gas) KCI H20 (water) HCI also explain how you got the answer, thanks.

Answers:There are alot of ways to answer this question. For instance, you could electronegativities of each element to calculate the Pauling dipole moment of the molecule and hence determine the type of bond. However, this looks like a grade school level question. The only way for you to really know which is ionic, covalent, or metallic is by knowing which elements share electrons and which transfer electrons. You should know which are metallic bonds because only transition metals like Fe (viz. iron) form metallic bonds. Covalent bonds form between elements that have similar electronegativities such as Carbon and Hydrogen ( C-H bonds). Ionic bonds form between elements of larger differences in electronegatives such as Potassium and Chlorine [K+][Cl-]. You should be able to figure the answer out from this.

Question:Ionic and Covalent Bonding? 1. Determine if the following compounds are likely to have ionic or covalent bonds. a. magnesium oxide, MgO b. Strontium chloride, SrCl2 c. Ozone, O3 d. Methanol, Ch4 O 2. Identify which 2 of the following substances will conduct electricity, and explain why. a. aluminum foil b. sugar, C12H22O11, dissolved in water. c. potassium hydroxide , KOH, dissolved in water 3. Draw the structural formula fir acetylene. Atoms bond in the order HCCH. Carbon and hydrogen atoms share 2 electrons, and each carbon atoms must have a total of four bonds. How many electrons do the carbon atoms share? 4. Predict whether a silver coin can conduct electricity. What kind of bonds does silver have? 5. Describe how it is possible for calcium hydroxide, Ca(Oh)2, to have both ionic and covalent bonds. 6. Explain why electrons are shared equally in ozone, O3, and unequally in carbon dioxide, Co2. 7. Analyze whether dinitrogen tetroxide, N2O4, has covalent or ionic bonds. Describe how you reached this conclusion. 8. Bond energy measure the energy per mole of a substance needed to break a bond. Which element has the greater bond energy, oxygen or nitrogen? (Hint: Which element has more bonds?) Answer as much as you can please.

Answers:1. Determine if the following compounds are likely to have ionic or covalent bonds. a. magnesium oxide, MgO ionic (metal and nonmetal) b. Strontium chloride, SrCl2 ionic (metal and nonmetal) c. Ozone, O3 covalent d. Methanol, CH4O covalent (C and O are nonmetals and H is a metal) *a metal bonded with a nonmetal forms an ionic bond; also, when an element is bonded to itself it forms a covalent bond 2. Identify which 2 of the following substances will conduct electricity, and explain why. a. aluminum foil because Aluminum is a metal and metals are highly conductive & c. potassium hydroxide, KOH, dissolved in water because potassium hydroxide dissolved in water dissociates and forms potassium and hydroxide ions; ions conduct electricity *It CAN'T be b. because sugar does not break up into ions that conduct electricity. 3. How many electrons do the carbon atoms share? Each carbon atom has 4 valence electrons, so each C atom can form 4 bonds. In HCCH, each carbon atom shares 4 electrons and sincethere are 2 of them, there are 8 electrons being shared. 4. Predict whether a silver coin can conduct electricity. What kind of bonds does silver have? The bonds between atoms are metallic which means that the outer electrons are held by weak bonds which can easily dissociate. Dissociation of ions causes electrical conductivity. 5. Describe how it is possible for calcium hydroxide, Ca(OH)2, to have both ionic and covalent bonds. Ca and O can share electrons (covalent bond) with each other or H can take electrons away (ionic bond) from Ca. 6. Explain why electrons are shared equally in ozone, O3, and unequally in carbon dioxide, CO2. In CO2, O is more electronegative meaning that it seeks to pull the electron between itself and carbon more strongly which results in unequal sharing of electrons. In O3, when atoms are bonded together, the electrons are shared equally. 7. Analyze whether dinitrogen tetroxide, N2O4, has covalent or ionic bonds. Describe how you reached this conclusion. N2O4 has covalent bonds because N and O are both nonmetals; nonmetals form covalent bonds. 8. Which element has the greater bond energy, oxygen or nitrogen? (Hint: Which element has more bonds?) Oxygen can form 6 bonds, but Nitrogen can only form 5 bonds, so Oxygen has a greater bond energy.

Question:Science wise.

Answers:Chemical Bonding Chemical compounds are formed by the joining of two or more atoms. A stable compound occurs when the total energy of the combination has lower energy than the separated atoms. The bound state implies a net attractive force between the atoms ... a chemical bond. The two extreme cases of chemical bonds are: Covalent bond: bond in which one or more pairs of electrons are shared by two atoms. Ionic bond: bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other. Other types of bonds include metallic bonds and hydrogen bonding. The attractive forces between molecules in a liquid can be characterized as van der Waals bonds. -x-x-x-x-x-x IONIC BOND: are forces that hold ionic compounds together If a negative ion meets a positive one, their opposite charges attract strongly and glue the atoms together. This type of gluing is called an ionic bond. Ionic bonds were first formed as atoms emerged from a supernova, and caused cosmic dust grains to form. They are important in holding the atoms together in many rocks on the Earth today. An ionic bond is sometimes called an electrovalent bond. COVALENT BOND: this major type of bond holds atoms together - A covalent bond is formed when the electron clouds of two atoms overlap. Where the clouds overlap they are thicker, and their electric charge is stronger. Both nuclei feel a force of attraction towards this thick electron cloud, and so the two atoms are held together. A group of atoms joined in this way is known as a molecule. The number of covalent bonds which an atom can form depends on how many electrons it has. The shell model explains this. METALLIC BOND: The properties of metals suggest that their atoms possess strong bonds, yet the ease of conduction of heat and electricity suggest that electrons can move freely in all directions in a metal. The general observations give rise to a picture of "positive ions in a sea of electrons" to describe metallic bonding.

From Youtube

Ionic and Covalent Bonding :This was a school project for science class that everyone wanted me to put on Youtube... and finally I found enough patience to do so

Ionic and covalent bonding animation :Ionic bonding formed when one atom has sufficient strength of attraction to remove ion from the other atom. Covalent bonding occurs when neither atom has sufficient strength to remove the other atom's electron. They would instead share electrons to form stable configurations of electrons.