General Chemistry: Electronic and Atomic Structure; Periodic Table

Question 1

iThe property defined as the energy required to remove one electron from an atom in the gaseous state is:

A. electronegativity C. electron affinity
B. ionization D. hyperconjugation

Answer 1

B. Ionization energy (IE) is the amount of energy required to remove the most loosely bound electron of an isolated gaseous atom to form a cation. This is an endosthermic process.
Ionizatioan energy is expressed as: X + energy (right arrow) X+ +e-
where X is an atom or molecule capable of being ioized (having electron removed), X+ is the atom or molecule after an electron is removed, and e- is the removed electron
The principle quantum number (n) describes the size of thenucleus. It refers to the sixe of the orbital and the energy level an electron.

The element with larger shell sizes (n is large) listed at the bottom of the periodic table have low ionization energies.

Question 2

Which of the following elements most easily accepts an extara electron

A. He C. Cl

B. Ca D. Fr

Answer 2

C. Accepting electrons to form anions is a characteristic of non-metals to obtain the electron configuration of the noble gases ( i.e., complete octet
Except helium which has a complegte ocatet with 2 electrons. 1s2, the noble gases have complete octet with ns2 and np6 orbitals.

Question 3

Which of the following pairs has one metalloid element and one nonmetal element

A. 32 Ge and 9 F C. 51 Sb and 20 Ca

B.19K and 9 F D. 33 As and 14 Si

Answer 3

A. Metalloids are semimetallic elements ( between metals and non metals). The metalloids are borons (B), silicon (Si), germanium (Ge), arsenic (As), antimony ( Sb) and tellirium ( Te).
nonmetals hydrogen, helium, notrogen, oxygen, fluorine, neon, chlorine, argon, kryptom, xenon, and radon
bromine a liquid,
solid: carbon, phosphorous, sulfur, seleenium, and iodine

Question 4

Periods on the periodic table represent elements:

A. in the same group C. known as isotopes

B. with consecutive atomic number D. with similar chemical properties

Answer 4

B.

Question 5

How many electrons can occupy the n=2 shell

A. 2 C. 8

B. 6 D.18

Answer 5

C. for n=2 shell, it has 2 orbitals: s, p
Each orbital can hold two electrons
The maximum number of electrons in each shell:

The s subshell has 1 speherical orbital and accomondate 2 electrons
The p subshell has 3 dumbbell-shaped orbitals and can accomondate 6 electrons
Maximum number of electrons in n=2 shell is: 2 (for s) + 6 ( for p) =8

Question 6

Ignoring hydrogen and helium which areas of the periodic table contains both metals and nonmetals

Answer 6

B.

Question 7

What is the number of known nonmetals relative to the number of metals