Lecture

Question 1

Atomic weight of carbon

Answer 1

12.0107

Question 2

Focus of inorganic chemistry

Answer 2

It is the general study of chemicals / elements.

Question 3

Focus of organic chemistry

Answer 3

It is specific to the study of CARBON and to all substances containing it.

Question 4

Source of molecules in inorg

Answer 4

Minerals

Question 5

Source of molecules in organic chemistry

Answer 5

Biological species (animals, plants)

Question 6

Atomic number gives the ?

Answer 6

of protons / electrons

Question 7

Mass number gives the ?

Answer 7

total # of protons and neutrons in the nucleus.

Question 8

Where can you find the negatively charged electron

Answer 8

Within the orbitals

Question 9

Atomic orbitals is also known as?

Answer 9

Wave function

Question 10

What is atomic orbitals

Answer 10

It is the solution to a wave equation — the mathematical expression used to describe the distribution of electrons in an atom.

Question 11

shape of s orbital

Answer 11

Spherical

Question 12

Shape of p orb

Answer 12

Dumbbell shape

Question 13

Hund’s principle -

Answer 13

states that every orbital in a subshell is singly occupied before other orbitals are completely filled and that electrons in a singly occupied orbital will have the same spin

Question 14

Aufbau’s principle

Answer 14

• states that electrons will fill the lowest available energy level before filling the higher levels

Question 15

Octet rule

Answer 15

states that the valence shell (outermost shell) must be filled completely and must achieve a noble gas configuration (8 valence electron).

Question 16

Atoms will achieve noble gas configuration by either

Answer 16

Forming ionic bond or covalent bond.

Question 17

Electrons are transferred

Answer 17

Ionic bond

Question 18

Electrons are shared

Answer 18

Covalent bond

Question 19

Bond between atoms of different
eletronegativity (cations and anions)

Answer 19

Ionic bond

Question 20

Bond (occurrence) covalent

Answer 20

Between similar atoms and atoms of
nearly equal electronegativity.

Question 21

shows the kernel or nucleus represented by the symbol of the atom surrounded by its valence electrons represented by dots.

Answer 21

Lewis dot structure

Question 22

also known as line-bond structures; shows 2- electron covalent bonds as a line and the lone-pair electrons (non- bonding electrons) as dots.

Answer 22

Kekúle structure

Question 23

Define electronegativity

Answer 23

a measure of the relative attraction an atoms has for the shared electron in a bond.

Question 24

The most electronegative

Answer 24

Fluorine

Question 25

Electronegativity of CNOF

Answer 25

C- 2.5 N- 3.0 O- 3.5 F- 4.0

Question 26

a measure of the degree of inequality in the sharing of electrons between two atoms in a chemical bond.

Answer 26

Bond polarity

Question 27

Non- polar covalent bond

Answer 27

a covalent bond in which there is a equal sharing of electrons between two atoms.

Question 28

is a covalent bond in which there is an unequal sharing of electrons between two atoms.n

Answer 28

Polar covalent bond

Question 29

Electronegativity difference of non polar

Answer 29

0-0.4

Question 30

Electronegativity difference of polar

Answer 30

0.4-1.5

Question 31

the no. of valence electrons in the neutral atom minus the number of covalent bonds to the atom and the number of unshared electrons on the atom.

Answer 31

Formal charge

Question 32

Formula for normal charge

Answer 32

Formal Charge = no . of valence e ! in neutral atom minus (no . of dots + no . of bonds)

Question 33

ground state electron configuration of carbon:

Answer 33

1s2 2s2 2p2

Question 34

Shape of sp3

Answer 34

Tetrahedral 109.5*

Question 35

Shape of sp2

Answer 35

Trigonal planar 120*

Question 36

Shape of sp

Answer 36

Linear 180

Question 37

Overlapping type for sigma bond

Answer 37

Head-on-overlap

Question 38

Overlapping type for pi bond

Answer 38

Sideway overlap

Question 39

forms when 2s orbital hybridize with 3 2p orbitals forming four (4) sp3 hybrid orbitals.

Answer 39

Sp3

Question 40

forms when 2s orbital hybridize with 2 2p orbitals forming three (3) sp2 hybrid orbitals and one (1) unhybridized p-orbital.

Answer 40

Sp2 carbon

Question 41

forms when 2s orbital hybridize with 1 2p orbital forming two (2) sp hybrid orbitals and two (2) unhybridized p-orbitals.

Answer 41

Sp carbon