General Inorganic Chemistry

electron

Arrange the proton, neutron and electron in increasing mass

a. proton< electron< neutron

b. electron< proton< neutron

c. electron< neutron< proton

d. neutron< electron< proton

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Balmer constant

The constant known as the fundamental number of hydrogen is the __________.

a. Rydberg constant

b. Planck's constant

c. Fine-structure constant

d. Balmer constant

the atom is almost an empty space

In Rutherford's experiment, which of the following is true?

a. the proton is evenly distributed in the nucleus of an atom

b. the atom is almost an empty space

c. the nucleus contains proton, neutron and electron

d. all of these

orbital

The region in space where an electron is most likely to be found is called

a. orbital

b. energy level

c. shell

d. nucleus

isotopes

Atoms with the same atomic number but different mass number is called

a. isobars

b. isotopes

c. isotherms

d. isoelectronic

Angular Momentum Quantum Number

The quantum number that has an allowable value of 0,1,2, etc. is the

a. Magnetic Quantum Number

b. Spin Quantum Number

c. Angular Momentum Quantum Number

d. Principal Quantum Number

Pauli's Exclusion Principle

It states that no two atoms will have the same set of quantum numbers

a. Heisenberg Uncertainty Principle

b. Pauli's Exclusion Principle

c. Aufbau Building Up Principle

d. Hund's Rule of Multiplicity

nuclear

Which of the following properties do not depend on the electronic configuration of the atoms?

a. physical

b. chemical

c. nuclear

d. none of the above

n=1, l=0, ml=-1, ms=-1/2

Which of the following sets of quantum numbers is incorrect?

a. n=1, l=0, ml=-1, ms=-1/2

b. n=1, l=0, ml=0, ms=1/2

c. n=3, l=1, ml=0, ms=-1/2

d. n=4, l=2, ml=-1, ms=1/2

5A

In what group of the periodic table is the element with the following electron configuration [Ar] 4s1 3d10 4p3

a. 1A

b. 2A

c. 3A

d. 5A

S^-2 and Cl^-1

Which of the following pairs are isoelectronic?

a. Mn^+2 and Ar

b. Zn^+2 and Cu^+2

c. S^-2 and Cl^-1

d. Na^+ and Cl^-1

Electron Affinity

The change in energy when an electron is accepted by a gaseous atom to form an anion.

a. Electronegativity

b. Electron Affinity

c. Ionization Energy

d. Activation Energy

F

Which of the following halogens is the most electronegative

a. F

b. Cl

c. Br

d. I

Oxygen

Among the members of the Chalcogen Family, which is the most non-metallic?

a. Sulfur

b. Selenium

c. Tellurium

d. Oxygen

23415

Arrange the following in increasing ionization energy:

C - 1, Na - 2, Mg - 3, B - 4, N - 5

a. 41532

b. 51432

c. 23415

d. 23514

Valence Bond Theory

the theory that states that bonding is caused by overlapping of two atomic orbitals.

a. Valence Bond Theory

b. Molecular Orbital Theory

c. Vital Force Theory

d. Valence Shell Electron-Pair Repulsion

Bond order

It pertains to single bond, double bond, triple bond and those intermediate between single and double bonds, etc.

a. Bond Order

b. Bond Length

c. Bond Strength

d. Bond Degree

(CH3)3COCH3

A compound whose molecules are not associated by hydrogen bonding is

a. CH3CH2OH

b. (CH3)2NH

c. HCOOH

d. (CH3)3COCH3

BeCl2

Which of the following molecules/compounds is formed by covalent bonds?

a. LiF

b. MgO

c. ZnS

d. BeCl2

homogeneous equilibria

Type of equilibrium that exists between similar phases is called

a. physical equilibria

b. homogeneous equilibria

c. chemical equilibria

d. heterogeneous equilibria

add PCl5

Consider the reaction: PCl5(g) <=> PCl3(g) + Cl2(g) 🔺H°rxn = 87.9 kj/mol

Which of the following will result in the increase in concentration of Cl2 gas?

a. add PCl3

b. cool the mixture

c. add PCl5

d. increase the pressure

sodium chlorite

NaClO2 is

a. sodium chloride

b. sodium hypochlorite

c. sodium chlorite

d. sodium chlorate

Na2C2O4

oxalic acid + sodium hydroxide -----> __________ + H2O

a. Na2CO3

b. NaC2H3O2

c. NaCHO

d. Na2C2O4

SO2

which of the following is an acidic oxide?

a. MgO

b. SO2

c. Na2O

d. CaO

Na2SO4

Which of the following substances in aqueous solution of the same concentration will have the highest boiling point elevation?

a. KCl

b. Na2SO4

c. CH3COOH

d. NaCl

alpha

If 238U92 undergoes decay and found to produce 234Bi90, what other particle was emitted?

a. alpha

b. gamma

c. positron

d. electron

curie

It is equivalent to the rate of disintegration of 1 gram of radium

a. becquerel

b. curie

c. gray

d. rem

neutron

Which of the following particles cannot be accelerated in a particle accelerator?

a. alpha

b. electron

c. neutron

d. proton

atoms

elements are composed of tiny indivisible particles called

Law of Multiple Proportions

If two elements combine to form more than one compound, the ratio of the mass of an element to a fixed mass of the other element is a whole number or a simple fraction

Law of Conservation of Mass

A chemical reaction only involves separation, combination or rearrangement of atoms

Law of Definite Proportions

states that a pure compound is made up of elements in the same proportion by mass.

Atomic number

is the number of protons in the nucleus of an atom.

Mass number

is the total number of protons and neutrons in the nucleus of an atom

Average atomic mass

of an element is the weighted average of the atomic masses of the isotopes based on their percentage abundance

Principal quantum number

pertains to the average distance of the electron from the nucleus in a particular orbital. It has integral values 1,2, etc.

Magnetic quantum number

describes the orientation of orbitals in space. Its allowable values are -l to 0 to +l

Spin quantum number

shows the spin of electrons. its values are +1/2 (clockwise) and -1/2 (counter clockwise)

Aufbau Principle

the orbitals of an atom must be filled up in increasing energy levels

Hund's Rule of Multiplicity

the most stable arrangement of electrons in subshells is the one with more parallel spins

Modern Periodic Law

the properties of the elements are functions of their atomic numbers

Atomic size (atomic radius)

is the average distance between the nucleus and the valence electron

Ionization energy

is the energy required to remove an electron from a gaseous atom in its ground state. The lower the IE, the easier it is for an atom to form a cation

Electronegativity

is the measure of the ability of an atom to attract towards itself a bonding electron

Covalent bond

results from the attraction of the nucleus and the electron of two or more atoms and usually involves two non-metals

Ionic Bond

results from the attraction of two opposite charged particles and involves a metal and a non-metal

Bond energy

is the amount of energy involved in the formation and breaking of a bond

Bond length

is the distance between the nuclei of the atoms forming the bond

Valence bond theory

the formation of a bond is due to the overlap of two atomic orbitals

Molecular orbital theory

a bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-bonding molecular orbital

Le Chatelier's Principle

a system in equilibrium when subjected to a stress will act in such a way to relieve the stress

Conservation of mass number

the total number of protons plus neutrons in the products and in the reactants must be the same

Conservation of atomic number

the total number of nuclear charges in the products and in the reactants must be the same