List and give an example of an object around you for of each of the different types of chemical bonds.
A chemical bond is any force of attraction that holds two atoms or ions together. [ In most cases, that force of attraction is between one or more negatively charged electrons held by one of the atoms and the positively charged nucleus of the second atom. Chemical bonds vary widely in their strength, ranging from relatively strong covalent bonds (in which electrons are shared between atoms) to
very weak hydrogen bonds. The term chemical bond also refers to the symbolism used to represent the force of attraction between two atoms or ions. For example, in the chemical formula H—O—H, the short dashed lines are known as chemical bonds.
Theories of chemical bonds go back a long time. One of the first was developed by Roman poet Lucretius (c. 95–c. 55 B.C. ), author of De Rerum Natura (title means "on the nature of things"). In this poem, Lucretius described atoms as tiny spheres with fishhook-like arms. Atoms combined with each other, according to Lucretius, when the hooked arms of two atoms became entangled with each other.
Words to Know
Covalent bond: A chemical bond formed when two atoms share one or more pairs of electrons with each other.
Double bond: A covalent bond consisting of two pairs of electrons.
Electronegativity: A numerical method for indicating the relative tendency of an atom to attract the electrons that make up a covalent bond.
Hydrogen bond: A chemical bond formed between two atoms or ions with opposite charges.
Ionic bond: A chemical bond formed when one atom gains and a second atom loses electrons. An ion is a molecule or atom that has lost one or more electrons and is, therefore, electrically charged.
Multiple bond: A double or triple bond.
Polar bond: A covalent bond in which one end of the bond is more positive than the other end.
Triple bond: A covalent bond consisting of three pairs of electrons.
Such theories were pure imagination, however, for many centuries, since scientists had no true understanding of an atom's structure until the beginning of the twentieth century. ]
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