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Chemistry 001 > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What is Chemical Bonding?

A

Chemical bonding refers to the attractive forces that hold atoms together in a compound.

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2
Q

What is Lewis Electron Don structure of an Atom?

A

A representation the valence electrons of an atom or molecule using dots.

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3
Q

What is Ionic (Electrovalent) Bonding?

A

The bond formed by the electrostatic attraction between cation and anion
-involves the transfer of one or more electrons from a metal to a nonmetal with the formation of ions.

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4
Q

What factors favour ionic bonding

A

I)Low ionization energy for the electron-donating atom
II) High electron affinity of the electron-accepting atom that is nonmetal
III) High lattice energy of the resultant ionic compounds.

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5
Q

What is Bond Energy?

A

The average amount of energy associated with making or breaking one mole of a particular bond in its gaseous state

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6
Q

What is Lattice Energy?

A

The energy required to separate 1mole of ions of an ionic compound

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7
Q

NOTE

A

-The greater the lattice energy the
stronger the force of attraction.
-Lattice energy is directly related to the size of the ions
bonded. Smaller ions form compounds with more closely spaced ionic charges. Because
the electrostatic force of attraction between opposite charges increases as the distance
between the charge decreases, smaller ions produce stronger interionic attraction and
greater lattice energies

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8
Q

What effect does the charge of the ion have on Lattice Energy

A

The ionic bond
formed from the attraction of ions with larger positive or negative charges generally has a
greater lattice energy

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9
Q

What are the general properties of Ionic Compounds

A

1) Exist as crystalline solids at ordinary temperatures
2) High melting and boiling point due to strong electrostatic attraction
3) When in molten or when dissolved in water , they can conduct electricity
4) Soluble in water and other polar liquid.
5) Ionic compound compound are generally insoluble in non polar liquids
6) Ionic crystals do not conduct electricity since the ions are trapped in a fixed place
7) They are often formed between two elements with quite different
electronegativities usually a metal and non metal

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10
Q

What is covalent Bonding

A

Covalent bonding involves the sharing of one or more pairs of electrons between two atoms of either the same element or two different elements.

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11
Q

What is Coordinate (Dative Covalent) Bonding

A

Coordinate bond is a type of covalent bond between two atoms in which the bonding
electron is supplied by one of the two atoms

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12
Q

What factors affect the strength of Covalent Bonds

A

The strength of a covalent bond depends on the distance between the bonded nuclei

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13
Q

What is bond length?

A

The distance between the two bonded nuclei at the position of maximum attraction
- As the number of shared electron pairs increases the bond length decreases

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14
Q

What is the relationship between bond length and bond strength

A

The shorter the bond length the stronger the bond.

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15
Q

What is the dissociation energy?

A

The amount of
energy required to break a specific covalent bond

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16
Q

What is Bond Polarity?

A

Bond polarity is a measure of how equally or unequally the electrons in any covalent bond are shared.

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17
Q

What is a non-polar covalent bond?

A

A bond in which the electrons are
shared equally
e.g. Cl₂ and N₂

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18
Q

What is a polar covalent bond?

A

A bond where one of the atoms exert a greater attraction for the bonding electrons than the other.

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19
Q

What determines the type of bond formed?

A

The electronegativity

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20
Q

What difference in electronegativity do non-polar covalent compounds have

A

Less than 0.4

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21
Q

What difference in electronegativity do polar covalent compounds have

A

Between 0.4 to 1.7.

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22
Q

What difference in electronegativity do ionic compounds have

A

Greater than 1.7

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23
Q

What is Fajan’s Rules of Bond Type?

A
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24
Q

What is the Octet Rule

A

The rule states that the most stable electron configuration of an atom occurs when that atom acquires the valence electron configuration of a noble gas

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25
Know how to draw Lewis Dot Structure
26
What are the exceptions to the Ocect Rule
-Molecules and polyatomic ions containing an odd number of electrons -Molecules and polyatomic ions in which an atom has fewer than an octet of valence electron - Molecules and polyatomic ions in which an atom has more than an octet of valence electron
27
Why are odd numbers an odd number of electrons an exception to the rule?
The number of valence electrons is odd in a few molecules and polyatomic ions such as ClO₂, NO, NO₂, and O₂. The complete pairing of these electrons is impossible and an octet around each atom cannot be achieved
28
Why is having less than an octet of valance electrons an exception to the rule?
29
What are formal changes?
Formal charge is the hypothetical charge on an atom in a molecule or polyatomic ion
30
What are the properties of Covalent Compounds
-At room temperature, covalent compounds are usually gases, liquids or low-melting point solid -Many are insoluble in polar solvent Most are soluble in non-polar solvents such as hexane
31
What are Sigma (σ) Covalent Bonds
A bond formed by the overlap of orbitals in an end-to-end or linear fashion with the electron density concentrated between the nuclei of the bonding atoms
32
How are sigma orbitals formed
I)By the overlap of two s-orbitals ii) By the overlap of p and s-orbitals iii) By the overlap of two p orbital
33
What are Pi (π) Covalent Bonds?
Pi bond is a bond formed by the overlap of orbital in a side by side or parallel fashion with the electron density concentrated above and below
34
What is the difference between sigma and pi covalent bonds?
Sigma bonds are stronger and there are not easily broken while pi bond are less strong and there are easily broke
35
What is Hybridization
Hybridization is the mixing or blending of two or more different types of orbitals of the same energy level to produce the same number of identical hybrid orbital
36
What is sp Hybridization
This is as a result of mixing the 2s and 2p orbital as in the case of BeCl2
37
sp² Hybridization
This is as a result of mixing 2s and two 2p orbitals to form three identical sp2 hybrid orbital as in the case of BF3.
38
What is sp³ Hybridization
This is as a result of mixing 2s and three 2p orbital to produce four equivalent sp³ hybrid orbital as in the case of methane (CH₄)
39
What is sp³d Hybridization
This is as a result of mixing 3s three 3p orbitals and 3d orbital to produce five equivalent sp³ d hybrid orbitals as in the case of phosphorus pentachloride (PCl₅)
40
What is sp³d² Hybridization?
This is a result of mixing 3s, three 3p orbitals, and two 3d orbitals to produce six equivalent sp³d² hybrid orbitals as in the case of SF₆.
41
What is the VESPR Model
The Valence Shell Electron Pair Repulsion (VSEPR) Model is usually a satisfactory method for predicting molecular shapes
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What are Intermolecular Forces ?
These are forces of interaction between molecules
45
What are Vander Waals Forces?
Collectively, forces between molecules 1) Molecules with Permanent Dipoles ( Dipole- Dipole forces) 2) Polar molecules with non polar ones( Dipole – induced dipole forces) 3) Non polar molecules ( induced dipole -induced dipole , also known as London forces or Dispersion
46
What is a dipole +
Refers to a separation of electric charge between two atoms or regions in a molecule, creating two poles: a positive pole (partial positive charge) and a negative pole (partial negative charge).
47
What are Dipole -Dipole Forces
An attractive intermolecular force resulting from the tendency of polar covalent molecules to align themselves in such a way that the positive end of one dipole is near the negative of another dipole
48
What are Dipole-Induced Forces?
The electron cloud of nonpolar molecules could easily be distorted when close to the positive end of a dipole. The electron cloud will be drawn toward the permanent dipole, this disturbs the electron cloud in the non-polar molecules and this induced a dipole
49
What are Induced Dipole- Induced Dipole (Dispersion or London forces)?
50
WHat is a Hydrogen Bond
Hydrogen bond is a dipole dipole intermolecular attraction which occur when hydrogen is covalently bonded to highly electronegative elements of small atomic size
51
What is melting point in chemistry
The change from the highly ordered arrangement of particles in the crystalline lattice to the more random arrangement that characterizes a liquid
52
Effect of Intermolecular Forces on Melting Point?
53
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57
What is a metallic bond
A chemical bond in which metals that consist of positive cores of atoms are held together by a surrounding electron cloud or sea of electrons
58
What is responsible for the conductivity of a metal?
The freedom of the electrons to move throughout the crystal
59
What are the structures of Metal
A) Close -Packed Structure: -Hexagonal close packing Zn, Mg) -Face centered cubic close packing (Cu, Al, Ag, Au) B) Body Centered Cubic (Fe, Cr)
60
What are the properties of a metallic compound
-Metals are good conductor of heat and electricity -Pure metals are malleable and ductile -Pure metals have a high melting point

Chemistry 001 (8 decks)

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