Bonding Flashcards

1
Q

Co-ordinate bond

A

A co-ordinate (dative covalent) bond contains a shared pair of electrons with both electrons supplied by one atom

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2
Q

Covalent bond

A

A shared pair of electrons between two non-metals

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3
Q

Dipole

A

Difference in charge between the two atoms of a covalent bond caused by a shift in electron density in the bond due to the electronegativity difference between elements participating in bonding

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4
Q

Electron pair repulsion

A

Repulsion that exists between electron pairs due to the negatively charged electrons. This repulsion means electron pairs position themselves as far apart from each other as possible around the central metal atom

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5
Q

Electronegativity

A

The power of an atom to attract the electron density in a covalent bond towards itself

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6
Q

Electrostatic forces

A

The strong forces of attraction between oppositely charged ions

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7
Q

Hydrogen bonding

A

An interaction between a hydrogen atom and an electronegative atom, commonly nitrogen, fluorine or oxygen. The slightly positive hydrogen is attracted to the lone pair on the electronegative atom. Hydrogen bonds are stronger than van der Waals and dipole-dipole forces but weaker than ionic and covalent bonds

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8
Q

Intermolecular forces

A

The forces which exist between molecules. The strength of the intermolecular forces impact physical properties like boiling/melting point

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9
Q

Ion

A

An atom of molecule with an electric charge due to the loss or gain of electrons

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10
Q

Ionic bond

A

A metal atom loses electron(s) to form a positively charged ion and a non-metal atom gains these electron(s) to form a negatively charged ion. An ionic bond is formed between the oppositely charged ions

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11
Q

Ionic compound

A

Chemical compound formed of ions, held together by strong electrostatic forces

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12
Q

Lattice

A

a repeating regular arrangement of atoms/ions/molecules. This arrangement occurs in crystal structures

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13
Q

Macromolecular crystal structure

A

Giant covalent structures. Macromolecules have very high melting points because many strong covalent bonds have to be broken. Examples include diamond and graphite

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14
Q

Metallic bonding

A

The bonds present in metals between the positive metal ions and negatively charged electrons

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15
Q

Permanent dipole-dipole forces

A

When molecules with polar covalent bonds interact with dipoles in other molecules dipole-dipole intermolecular forces are produced between the molecules. These intermolecular forces are generally stronger than van der Waals forces but weaker than hydrogen bonding

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16
Q

Polar bond

A

A covalent bond between two atoms in which the electrons in the bond are unevenly distributed. This causes a slight charge difference, inducing a dipole in the molecule

17
Q

Simple molecular crystal structure

A

Structures in which atoms are joined by strong covalent bonds. Weak intermolecular forces mean simple molecules have low melting and boiling points

18
Q

Van der Waals

A

Also known as induced dipole-dipole, dispersion and London forces, van der Waals forces exist between all molecules. They arise due to fluctuations of electron density with a nonpolar molecule. These fluctuations may temporarily cause an uneven electron distribution, producing an instantaneous dipole. This dipole can induce a dipole in another molecule, and so on

19
Q

VSEPR theory

A

Valence shell electron pair repulsion theory is used to deduce the geometry of molecules. Pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repulsion. Lone pair-lone pair repulsion is greater than lone pair-bond pair repulsion, which is greater than bond pair-bond pair repulsion