ionic lattice?

Question

what is the ionic lattice?? is it the same as ionic bonding?
urgent help please

Answer 1

Ionic Bond

A chemical bond is a mutual attraction between the nuclei and valence electrons of two different atoms. This attraction results in the two atoms binding together. An ionic bond, also called an electron-transfer bond, is a type of chemical bond that is a result of the electromagnetic attraction between ions of opposite charges, i.e., a cation (a positively charged ion) and an anion (a negatively charged ion). An ion is an atom or group of atoms that has acquired an electrical charge due to the loss or gain of electrons. In an ionic bond, an atom gives or receives electrons from another atom. This is in contrast to covalent bonding, where two atoms share electron pairs between them. An ionic compound consists of anions and cations combined such that the total charge of the molecule is zero. All salts are ionic compounds.

One characteristic that both ionic and covalent compounds share is that they adhere to the octet rule. The octet rule is the principle that describes the bonding in atoms. Individual atoms are unstable unless they have an octet of electrons in their highest energy level. The electrons in this level are called valence electrons. When atoms gain, lose, or share electrons with other atoms, they satisfy the octet rule and form chemical compounds.

Ionic bonding occurs when one atom transfers electrons to another atom. In doing so, the atoms may achieve a complete outer energy level, satisfying the octet rule. During the formation of an ionic bond, one atom gains electrons and the other atom loses electrons. As a result, the atoms gain an electric charge. The atom that gains electrons gains a negative charge, becoming an anion. The atom that loses electrons gains a positive charge, becoming a cation. An example of this is the ionic bond that is formed between sodium (Na) and fluorine (F) to make sodium fluoride, NaF. A fluorine atom has seven valence electrons. It needs one more to have a complete outer energy level and satisfy the octet rule. If it gains this electron, it will become a negatively charged fluorine anion (F-). A sodium atom has only one valence electron. If it loses this electron, it is left with a complete outermost energy level that satisfies the octet rule. At the same time, it becomes a positively charged sodium cation (Na+). As the sodium atom loses its electron, the fluorine atom picks it up. The two ions now have opposite charges and attract each other. This electromagnetic attraction is quite strong and holds the ions together, forming sodium fluoride. This binding of the two ions is called an ionic bond.

Energy is required for an atom to lose an electron. The process of losing an electron and forming an ion is called ionization. The energy that is needed for ionization to occur is called the ionization energy. The ionization energy needs to be sufficient to overcome the attraction between the positively charged nucleus and the negatively charged electron. If an atom has only a few valence electrons, the ionization energy is low. The removal of a small number of electrons does not require much energy. Atoms with few valence electrons tend to lose these electrons easily and become cations. Sodium is an example of this phenomenon. A sodium atom only has one valence electron, which it loses quite easily. Thus, a sodium atom has a low ionization energy. In contrast, atoms with many valence electrons have high ionization energies. The removal of several electrons requires more energy. These atoms do not lose electrons easily, instead, they tend to gain electrons and become anions. An atom that gains electrons easily is said to have electron affinity. Fluorine is an example of an atom with electron affinity. A fluorine atom has seven valence electrons, so it does not lose electrons easily. Instead, it tends to gain an electron in order to complete its outermost energy level.

Most bonds are not completely ionic nor are they completely covalent. How ionic or covalent a chemical bond is depends on how strongly the atoms of each element attract electrons.Electronegativity (a measure of an atom's tendency to attract electrons) can be used to predict whether a bond will be a nonpolar covalent bond, a polar covalent bond, or an ionic bond. If the difference between the electronegativities of two atoms is 2.0 or greater, the bond is an ionic bond. If the difference is 0.4 or less, the bond is nonpolar. If the electronegativity difference between two atoms is between 0.4 and 2.0, the bond is considered to be a polar covalent bond. The greater the electronegativity difference, the greater the polarity, and the greater the ionic character of the bond.

Many substances are formed through ionic bonding. As mentioned above, all salts are formed with ionic bonds. A familiar example of an ionic compound is table salt, found in nature as rock salt. Table salt is sodium chloride (NaCl). A sodium ion, Na+, has a charge of 1+. A chloride ion, Cl-, has a charge of 1-. When a sodium atom gives up an electron to become Na+, and a chlorine atom gains this electron to become Cl-, these atoms combine as NaCl, forming an ionic compound with no electrical charge. The majority of the rocks and minerals found on the Earth are formed using ionic bonding.

An ionic compound has a specific structure. Most ionic compounds are crystalline solids. An ionic compound is composed of a network of ions that results in a three-dimensional matrix of cations and anions. This crystalline structure is an orderly arrangement of ions known as a crystal lattice. A crystal lattice structure minimizes an ion's potential energy. Therefore, this structure is energetically favorable. The arrangement of ions in a crystal lattice represent the optimum balance between the forces of attraction among oppositely charged ions and the forces of repulsion among ions of the same charge.

The physical arrangement of ions in a crystal lattice depends upon the number of ions as well as the sizes and charges of the ions. An ionic compound cannot be isolated into individual, neutral units, like a molecular compound can. The chemical formula of an ionic compound, therefore, does not represent the formula for one molecule of the substance. Instead, it represents the simplest ratio of the ions that gives the compound no net electrical charge. The chemical formula of an ionic compound represents one formula unit of the compound, i.e., the simplest combination of atoms that gives the compound electrical neutrality. The ratio of ions in a formula unit depends on the charges of the ions in the compound. For example, the ionic compound calcium fluoride is composed of calcium cations (Ca2+) and fluorine anions (F-). In order to have a net charge of zero, two fluorine atoms must combine for every calcium atom. This relationship is represented in the compound's chemical formula, CaF2.

The forces of attraction between ions in an ionic compound are very strong. The forces involved in ionic bonding are much stronger than the forces in a covalent bond. This difference in strength gives ionic compounds different properties than covalent compounds. The strong forces that hold ions together cause ionic compounds to have higher melting and boiling points than covalent compounds. Ionic compounds also do not vaporize as easily at room temperature as covalent compounds. Ionic compounds are very hard and also quite brittle, due to the crystal lattice structure. The ions in the crystal lattice cannot move very much without disturbing the overall balance between negative and positive charges. If one layer of atoms is moved, the result is a buildup of repulsive forces within the crystal structure, and the entire structure falls apart. Ionic compounds are good conductors of electricity when melted or dissolved in water because the ions dissociate in these states and are free to move and carry electrical current. In the solid state, the ions are not free to move, and the solid ionic compound does not conduct electricity.

Ionic compounds are found extensively in the Earth's crust. They are very strong structures with unique properties. The properties of ionic compounds, for example, electrical conductivity, can be exploited for use in science and technology. Research into the nature of ionic bonding continues in order to find new uses for these compounds.

Answer 2

Ionic Lattice

Answer 3

Ionic lattice, or crystal lattice, has to do with how many of the same molecule orient themselves in a solid. This is not the same as ionic bonding. Ionic bonding is the bonding of two atoms of different ionic charges, Na+ and Cl- = NaCl.

There are many different kinds of ionic lattices and the patterns they make depend on the complexity of the molecules and how much space they take up in orientation to another duplicate molecule in the solid.

Check out the following website for more information:

http://www.wou.edu/las/physci/ch412/lattice.html

Answer 4

possibly x-ray diffraction of a crystal of the ionic compound ? depending on which positive and negative ions you have then they pack into the structure in different proportions and different ways. I guess you could possibly also check density so mass and volume might come in useful here for calculations.

Answer 5

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RE:
ionic lattice?
what is the ionic lattice?? is it the same as ionic bonding?
urgent help please

Answer 6

Its the structure formed due to ionic bonding.

Answer 7

its the lattice of ion