Introduction: Inorganic & Organic Chemistry

Question 1

-Is defined as the chemistry of hydrocarbon compounds and their derivatives

Examples: soap, wood, paper, food

Answer 1

Organic Chemistry

Question 2

Can be described broadly as thechemistryof “everything else”

Examples: NaCl, water

Answer 2

Inorganic Chemistry

Question 3

play a vital role in living organisms.

•involved in a variety of processes within the human body. e.g.oxygen transport, formation of the framework for our bones.

Answer 3

Metal Ions

Question 4

an iron-containing metalloprotein which carries oxygen from the lungs to the various tissues around the human body.

Answer 4

Hemoglobin

Question 5

-a vital component of our bones.

Answer 5

Calcium (Ca) ions

Question 6

-essential for a variety of catalytic processes.

Answer 6

Elements such as copper (Cu), zinc (Zn) and manganese (Mn)

Question 7

What diagram illustrates the relationship between metal concentration and the body’s physiological response?

Answer 7

Bertrand diagram

Question 8

“All matter is composed of atomsand these cannot be made or destroyed. All atoms of the same element are identical and different elements have different types of atoms. Chemical reactions occur when atoms are rearranged.”

Answer 8

Dalton’s Atomic Theory

Question 9

In 1924, ______________ that all moving particles, especially electrons, show a certain degree of wave-like behavior. Therefore, he proposed the idea of wave-like nature of electrons, which became known as the ______________.

Answer 9

Louis de Brogli argued, phenomenon of the wave–particle duality

Question 10

published in 1926 the famous wave equation named after him.

Answer 10

Schrödinger

Question 11

f an electron has a wave-like consistency, there are important and possibly difficult-to-understand consequences; it is not possible to determine the exact momentum and the exact position at the same moment in time. This is known as

Answer 11

Heisenberg’s Uncertainty Principle

Question 12

Each atomic orbital is defined by a set of three quantum numbers:

Answer 12

the principal quantum number (n), the orbital quantum number (l) and the magnetic quantum number (ml).

Question 13

is the result of the radial part of the wave function being solved
￭can take values of 1 ≤ n ≤ ∞

Answer 13

Principal quantum number (n)

Question 14

represents the shape of the AO
￭is called the azimuthal quantum number, angular quantum number or orbital quantum number as it represents the orbital angular momentum of the electron
￭it can have values of l= 0, 1, 2, …, (n − 1), which correspond to the orbital labels s, p, d and f

Answer 14

S-Orbital Quantum number (l)

Question 15

￭Magnetic quantum number

￭provides information about the orientation (directionality) of the AO and can take values between +land −l

￭s-orbital only has one direction becausel = 0 ; ml= 0

Answer 15

Quantum number (ml)

Question 16

fourth quantum number: **_____________* s(value of either +1/2 or −1/2).

Answer 16

spin quantum number*

Question 17

“No two electrons in the same atom can have the same values for their four quantum numbers.”

Answer 17

Pauli Exclusion

Question 18

is defined as an electron that is part of an atom and can participate in the formation of a chemical bond. In main group elements, the valence electron is positioned in the outermost shell.

Answer 18

valence electron

Question 19

◇describes a set of electrons that occupy the same principal quantum number n

◇The respective electron shell n can be filled with 2n2electrons.

◇n=1; 2(11)= 2 electrons

◇n=2; 2(22)= 8 electrons

Answer 19

Electron shell

Question 20

◇are defined by the quantum numberl (l= n − 1), which as previously described correspond to the orbital labels s, p, d and f

◇The number of electrons that can be placed in each subshell can be determined by the following equation: 2(2l+ 1).

Answer 20

Electron subshells

Question 21

◇It describes the hypothetical process of filling the orbitals of an atom with the given number of electrons.

◇The first orbitals filled are the ones with the lowest energy levels before going onto the next higher energy level.

Answer 21

Hund’s Rule or Electron Subshell

Question 22

“Orbitals of the same energy level (such as p or d orbitals) are filled with one electron first before the electrons are paired within the same orbital.”

Answer 22

Hund’s Rule

Question 23

is the term used for the description of the electronic configuration of noble gases.

Answer 23

Noble gas configuration

Question 24

◇formation of ionic species was seen as a result of the transfer of electrons between atoms: anion (-) and cation (+)

◇covalently bonded molecules was described as a sharing of valence electrons

Answer 24

Bonds

Question 25

A **___________* is defined as an attraction between atoms, which leads to the formation of chemical substances containing two or more atoms. The bond is a result of the electrostatic attraction between opposite charges, such as electrons or nuclei or dipole attraction. Strong bonds: ionic bonds and covalent bondsWeak bonds: dipole interaction and hydrogen bonding

Answer 25

chemical bond

Question 26

are used to simply describe how valence electrons are arranged in molecules and how they are involved in chemical bonds.

Answer 26

Lewis structures

Question 27

◇are a set of rules used to predict the shape of a molecule ◇valence electrons around the center atom repel each other and will form an arrangement in which they are situated furthest from each other.

Answer 27

VSEPR(valence shell electron pair repulsion) rules

Question 28

are included in this electrostatic repulsion.

Answer 28

Lone pairs

Question 29

are seen the same as single bonds.

Answer 29

Double and triple bonds

Question 30

is defined as a chemical bond that is based on the sharing of electrons. Often, this leads to full outer shells for the binding partner to obtain the noble gas configuration.

Answer 30

covalent bond

Question 31

one bond partner would donate all the electrons needed to form the bond.

Answer 31

Dative covalent bond (coordinate)-

Question 32

chemical bond occurs between two atoms of the same element;the binding electron pair is evenly distributed between the two partners.

Answer 32

Homonuclearspecies

Question 33

chemical bond occurs between two atoms of different elements;the electrons are more attracted/polarized to one partner than the other, depending on electronegativity (EN).

Answer 33

heteronuclear species

Question 34

- describes the tendency of an atom to attract electrons or electron density towards itself. - depends on the atomic number and the distance of the valence electrons from the nucleus. - Pauling scale (most common)

Answer 34

Electronegativity

Question 35

describes the formation of a covalent bond as the overlapping of two half-filled valence AOs from each binding partner, which contains one electron each.

Answer 35

Valence Bond theory

Question 36

approaches chemical binding from a more advanced point of view, where MOs are formed covering the whole molecule.

Answer 36

Molecular orbital theory

Question 37

are strong bonds based on the transfer of electrons between the atoms and the resulting electrostatic attraction between the negatively and positively charged bond partners

Answer 37

Ionic Bond

Question 38

is used for atoms or molecules in which the total number of electrons is different from the number of protons and therefore carries a positive or negative charge.

Answer 38

ion

Question 39

◇a type of chemical bond where the metal atom donates its valence electrons to a ‘pool’ of electrons that surrounds the network of metal atoms ◇Electrons are not anymore identified with one particular atombut are seen as delocalized over a wide range.

Answer 39

Metallic Bond

Question 40

◇are the weakest forces occurring between molecules ◇They can be found between molecules that do not have a permanent dipole. ◇Electrons move around, leading to the formation of temporary dipoles. ◇Moleculesareweakly attracted to each other.

Answer 40

van der Waals forces

Question 41

◇is an electrostatic interaction of permanent dipoles ◇In heteronuclear molecules, a polarization of the bond is caused by the difference in electronegativity between the two atoms forming the covalent bond.

Answer 41

Dipole–dipole interaction

Question 42

◇seen as the particularly strong electrostatic interactions occurring between molecules of the type H-X ◇X is an electronegative atom such as F, O or N. ◇O and N have also the advantage of possessing lone-pair orbitals. ◇can be seen as a strong and specialized form of dipole–dipole interaction and is the reason for the high boiling point of water.

Answer 42

Hydrogen bonding