Comparing Ionic & Covalent Bonding

Comparing the Similarities and Differences of  Ionic vs. Covalent Bonding/Compounds Similarities:

1. Both types types involve involve multiple multiple atoms atoms coming togethe togetherr to form a more more complex complex structure. 2. In both types, types, bonding bonding yields yields a compoun compound d that has differen differentt properties properties than than the original elements. 3. Both types types of bonding bonding result result in atoms atoms becoming becoming more more stable in the group group than than they were individually. 4. Both Both type types s of bond bondin ing g are are exot exothe herrmic mic as the the pote potent ntia iall ener energy gy of the the participants is lowered as they form the bond. . Both types types of compounds compounds involve involve the interaction interaction between between valence valence electrons. electrons. !. In both types types of bonding bonding the attractiv attractive e force is an electrosta electrostatic tic one whereby whereby opposit opposite e charges charges attract " there there is no physica physicall matter matter holding holding the atoms atoms together. #. In the solid, crystalline crystalline state, both both types lead lead to regular, regular, ordered ordered patterns patterns and structures. $. Both types types of compound compounds s can undergo undergo changes changes in physica physicall state under under the right conditions of temperature and pressure. %. Both type types s of compound compounds s have have a net neutral neutral char charge. ge. 1&. 1&. Both Both type types s of comp compou ound nds s cont contai ain n a fixe fixed d rati ratio o of part partic icip ipan ants ts that that is represented by the subscripts in their chemical formulas 'they do not re(uire a 1)1 ratio*. Differences:

1. Ionic Ionic bonding bonding occurs between between atoms that have have opposite opposite needs for electrons electrons 'metal 'metals s and and nonme nonmetal tals* s* and and resu results lts in a transf transfer er of electr electron ons. s. +ova +ovalen lentt bonding occurs between atoms that have similar needs for electrons 'two nonmetals* and results in a sharing of electrons. 2. By trans transfer ferrin ring g elec electro trons ns,, ionic ionic bond bonding ing leads leads to the the format formation ion of charg charged ed particles that have either an excess of protons 'cation* due to the loss of  electrons or an excess of electrons 'anion* due to the gain of electrons. +ovalent compounds contain neutral atoms. 3. he electros electrostati tatic c attraction attraction that that occurs in ionic bonding bonding is between between cations cations and anions. he electrostatic attraction in covalent bonding arises from a shared electron-s attraction for its original nucleus as well as the nucleus of  the sharing atom. 4. Ions bond bond in a pattern pattern that maximies attractions attractions between between oppositely oppositely charged charged ions and minimies repulsions between li/e charged ions. he geometric pattern that arises is called the crystal crystal lattice and is consistent throughout throughout the crystal. 0ll ions are held by a networ/ of ionic bonds which are considered strong intramolecular forces. 0toms in a covalent compound are held together  by covalent bonds which are also considered strong intramolecular forces. owever, the atoms form distinct groups called molecules which are only wea/ly attracted to neighboring molecules by intermolecular forces. +hemistry

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. here is no distinctly individual unit in an ionic crystal. owever, there is a definite, fixed ratio between the cations and anions present. his ratio is used to come up with a 5formula unit6 which represents the base ratio by way of  subscripts '0l+l3*. he crystal itself may truly have 1 billion illion aluminum ions and 3 billion illion chloride ions. +ovalent compounds contain individual units called 5molecules6 that also have a fixed ratio of participants '+7 2*, however, the subscripts in this case represent the absolute number of atoms present in each molecule of the compound. !. It is more difficult to brea/ apart a salt because its structure is entirely strong intramolecular forces 'ionic bonds*. 8olecules only have strong intramolecular forces 'covalent bonds* holding the individual group together. he intermolecular attractions that can hold one molecule to its neighbor is wea/ therefore the molecules can be easily separated by increasing their  motion by raising their /inetic energy 'temperature*. 9alts have high melting and boiling points so that are found as solid crystals at normal conditions. 8olecules melt and boil at much lower temperatures. he everyday physical state changes that you notice in your surroundings are the molecules because they can melt, freee, evaporate, and condense at more normal temperatures. #. :ue to the fact that they are made up of charged particles, salts can conduct electricity when their ions are mobile 'molten or dissolved in water*. 8olecules are neutral and can not conduct electricity. hey may appear to conduct electricity if they react with water molecules to form ions 'called ioniation reaction*. $. ;lectron clouds overlap in covalent bonding. %. In covalent bonding, two atoms of the same element can bond together. 1&.here are more covalent compounds in nature than ionic. 11.
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