INORGANIC CHEMISTRY (LECTURE) Flashcards
The elements having an electron
configuration of ns2 np4 are called
d. chalcogens
The azide ion, N3–, is isoelectronic with
which of the following?
c. CO2
Number of elements in periodic table
118 elements
What group is s-Block in periodic table?
Group 1 & 2
What group is p-Block in periodic table?
Group 13 to 18
What group is d-Block in periodic table?
Group 3 to 12
core method : uses the closest and lower atomic number ____
Noble Gas
Electric Configuration four methods
a. Orbital Method
b. Shell Method
c. Core Method
d. Rectangular Arrow Method
Atomic number is equal to?
no. of protons
mass number is equal to?
no. of protons + no. of neutrons
elements with same atomic number but different
mass number or no. of neutrons
ISOTOPES
elements With the same number of electrons
ISOELECTRONIC
Elements with the same number of neutrons.
ISOTONES
elements With the same mass number
ISOBARS
pertains to the average distance of the electron from the nucleus in a particular orbital. It has integral values 1, 2, etc.
Principal Quantum Number (n)
tells the shape of the orbital. It has values from 0 to n - 1
Azimuthal/Angular Momentum Quantum Number (l)
describes the orientation of orbitals in space. Its allowable values are -l to 0 to +l
Magnetic Quantum Number (ml)
shows the spin of electrons. Its values are 1/2 ↑ (clockwise) and - 1/2 (counter clockwise)↓
Spin Quantum Number (ms)
If the electronegativity difference (usually called deltaEN) is less than 0.2, then the bond is
pure covalent
If the deltaEN is between 0.2 and 1.63, the bond is considered
polar covalent
If the deltaEN is greater than 1.63, the the bond is
lonic
Involves sharing of e- between two non-metals
Covalent Bond
Involves loss and gain of e- from metal and non-metal, respectively
Ionic Bond
ability of an atom to attract toward itself a pair of bonding electron
Electronegativity
Atomic size, Metallic Property, Reactivity
Increasing
Ionization energy, Electron affinity, Electronegativity
Decreasing
An atom in its free of elemental form has oxidation equal to
zero
For monoatomic ions, the oxidation number is equal to its
charge
Metals have ___ oxidation number
positive
Non- Metals usually have ___ oxidation number
negative
oxidation number of alkali metals: ___
+1
oxidation number of alkaline earth metals: ___
+2
oxidation number of aluminum: ___
+3
oxidation number of zinc: ___
+2
oxidation number of silver: ___
+1
Oxygen is usually -2, except in
peroxides (-1), and superoxides (-1/2)
Hydrogen is usually +1 except in
hydrides (-1)
Fluorine has __ oxidation state
-1
Other halogens are usually in the -1 oxidation state, except when combined with____, they are ____
oxygen; positive
The sum of oxidation number of elements in a compound is equal to
zero
The sum of oxidation number of elements in a polyatomic ion is equal to the
charge of the ion
Colligative properties of solution
-BPE, FPD, VPL, OP
KB (ebullioscopic constant) of water
0.5131 k/molal
KF (cryoscopic constant) of water
1.8605 k/molal
approaches the no. of ions in solution
i = vant hoff factor
as i (vant hoff factor) increase
colligative properties increase
