CTJan27 Online JMSS - Electrons Subshells and Periodic Tabel

1

What is the maximum number of electrons that can occupy the third principal energy level ($n=3$)?

$8$ $18$ $32$ $2$

2

The principal quantum number ($n$) primarily describes which characteristic of an electron's energy state?

The shape of the orbital. The spatial orientation of the orbital. The spin direction of the electron. The main energy level or shell.

3

Which subshells are present in the second principal energy level ($n=2$)?

$s$ only $s$, $p$, and $d$ $s$ and $p$ $s$, $p$, $d$, and $f$

4

What is the maximum number of electrons that can be held in an s subshell?

$6$ $2$ $10$ $1$

5

The p subshell contains how many individual orbitals, and therefore holds a maximum electron capacity of how many electrons?

1 orbital, 2 electrons 3 orbitals, 6 electrons 5 orbitals, 10 electrons 7 orbitals, 14 electrons

6

What is the maximum electron capacity of the d subshell?

$14$ $6$ $10$ $2$

7

Which geometric shape best describes the boundary surface of an s orbital?

Dumbbell Spherical Cloverleaf Pyramidal

8

The p orbitals are characterized by which shape and orientation set?

Spherical, oriented along one axis ($x$ only) Dumbbell, oriented along three perpendicular axes ($x, y, z$) Cloverleaf, oriented randomly Double dumbbell, oriented along five axes

9

Which principle dictates that electrons fill the lowest available energy levels before moving to higher ones?

Pauli Exclusion Principle Hund's Rule Aufbau Principle Heisenberg Uncertainty Principle

10

According to the diagonal rule (Aufbau principle), which subshell is filled immediately after the $3p$ subshell?

$3d$ $4p$ $4s$ $5s$

11

Comparing the energy levels, which statement is true according to the Aufbau filling order?

The $3p$ subshell has higher energy than $4s$. The $4s$ subshell has higher energy than $3d$. The $3d$ subshell has higher energy than $4s$. The $1s$ subshell has higher energy than $2s$.

12

The diagonal rule mnemonic (or 'rainy day' rule) visually organizes subshells based on increasing values of what combined characteristic?

Principal quantum number ($n$) only. Angular momentum quantum number ($l$) only. The sum of the principal and angular momentum quantum numbers ($n+l$). Magnetic quantum number ($m_l$) only.

13

The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of four quantum numbers. In practical terms, what does this limit imply for electrons occupying the same orbital?

They must have the same spin. They must occupy different subshells. They must have opposite spins. They must occupy different principal energy levels.

14

Hund's Rule of Maximum Multiplicity specifically governs how electrons fill orbitals within the same subshell (like $2p_x, 2p_y, 2p_z$). What is the requirement of Hund's Rule?

Electrons must pair up immediately to minimize energy. Orbitals must be filled completely before moving to the next subshell. Electrons occupy separate orbitals within a subshell with parallel spins before pairing. The maximum number of electrons per orbital is one.

15

Which configuration violates Hund's Rule?

Three electrons placed singly across the $2p$ orbitals. Two electrons placed in the first $2p$ orbital, and one electron placed in the second $2p$ orbital. Two electrons placed in the $1s$ orbital and two in the $2s$ orbital. Four electrons placed in the $2p$ subshell (three unpaired, one paired).

16

In the standard electron configuration notation ($1s^2 2s^2 2p^6$), what does the superscript number (e.g., $6$) represent?

The principal quantum number ($n$) The total number of electrons in that orbital. The maximum capacity of the subshell. The number of electrons occupying that specific subshell.

17

What is the ground state electron configuration for a neutral Nitrogen atom ($Z=7$)?

$1s^2 2s^2 2p^2 3s^1$ $1s^2 2s^3 2p^2$ $1s^2 2s^2 2p^3$ $1s^2 2p^5$

18

Determine the ground state electron configuration for Oxygen ($Z=8$).

$1s^2 2s^2 2p^5$ $1s^2 2s^4 2p^2$ $1s^2 2s^2 2p^4$ $1s^2 2s^2 3s^2 2p^2$

19

What is the ground state electron configuration for the noble gas Neon ($Z=10$)?

$1s^2 2s^2 3s^6$ $1s^2 2s^2 2p^6$ $1s^2 2s^2 2p^4 3s^2$ $1s^2 2s^4 2p^4$

20

Which configuration represents a neutral atom of Sulfur ($Z=16$)?

$1s^2 2s^2 2p^6 3s^2 3p^4$ $1s^2 2s^2 2p^6 3s^4 3p^2$ $1s^2 2s^2 2p^6 3d^6$ $1s^2 2s^2 2p^6 3s^2 4s^2$

21

Magnesium ($Z=12$) belongs to the alkaline earth metals. What is its electron configuration?

$1s^2 2s^2 2p^6 3s^1 3p^1$ $1s^2 2s^2 2p^8$ $1s^2 2s^2 2p^6 3s^2$ $1s^2 2s^2 2p^4 3s^4$

22

The configuration $1s^2 2s^2 2p^6 3s^1$ corresponds to which group on the periodic table?

Group 2 (Alkaline Earth Metals) Group 1 (Alkali Metals) Group 18 (Noble Gases) Group 17 (Halogens)

23

How many valence electrons does an atom with the electron configuration $1s^2 2s^2 2p^5$ possess?

$2$ $5$ $7$ $9$

24

Elements whose highest energy electrons are filling the p subshell are generally found in which block of the periodic table?

s-block d-block (Transition Metals) f-block (Inner Transition Metals) p-block

25

The electron configuration $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$ corresponds to which neutral atom?

Potassium ($Z=19$) Argon ($Z=18$) Calcium ($Z=20$) Zinc ($Z=30$)

26

Dmitri Mendeleev arranged the elements in his first periodic table primarily based on:

Atomic number ($Z$) Chemical reactivity Atomic mass Density at STP

27

The most significant contribution of Mendeleev to the historical development of the Periodic Table was:

Establishing the concept of isotopes Successfully predicting the properties of undiscovered elements Identifying the role of neutrons in the nucleus Using spectroscopy to identify new elements

28

Mendeleev predicted the existence of an element he called 'Eka-Aluminum'. This element was later discovered and named:

Germanium ($ ext{Ge}$) Scandium ($ ext{Sc}$) Gallium ($ ext{Ga}$) Technetium ($ ext{Tc}$)

29

Which scientist, working in the early 20th century, provided the experimental evidence that led to the organization of the modern Periodic Table based on atomic number ($Z$)?

Henry Moseley Ernest Rutherford John Dalton Antoine Lavoisier

30

The defining feature for ordering elements in the modern Periodic Table is the number of:

Neutrons in the nucleus Protons in the nucleus (Atomic Number, $Z$) Total electrons in the atom Mass number ($A$)

31

What is the term used to describe a horizontal row in the Periodic Table?

Group Family Block Period

32

The period number of an element in the main body of the Periodic Table corresponds to which atomic characteristic?

The number of protons The number of neutrons The total number of valence electrons The number of occupied main energy levels (shells)

33

How many elements are typically included in the 6th Period of the Periodic Table?

8 18 32 50

34

What is the term used to describe a vertical column in the Periodic Table?

Series Row Period Group or Family

35

Elements within the same group generally share the same:

Atomic mass Chemical properties Number of occupied energy shells Physical state at room temperature

36

The elements in Group 2 of the Periodic Table are commonly known as the:

Alkali Metals Alkaline Earth Metals Chalcogens Halogens

37

How many valence electrons does an element in Group 17 (excluding transition metals) typically possess?

1 2 7 8

38

Which classification group consists of elements that are typically shiny, malleable, ductile, and excellent conductors of heat and electricity?

Nonmetals Metalloids Metals Noble Gases

39

Elements that are brittle solids, poor electrical conductors, and tend to gain electrons in chemical reactions are classified as:

Alkaline Earth Metals Noble Gases Nonmetals Transition Metals

40

Where are metalloids primarily located on the standard Periodic Table?

Group 1 and 2 Along the zigzag dividing line (staircase) The bottom two rows (Lanthanides and Actinides) Groups 13 through 18 in the top periods only

41

Which of the following elements is classified as a metalloid?

Sulfur ($ ext{S}$) Calcium ($ ext{Ca}$) Boron ($ ext{B}$) Iron ($ ext{Fe}$)

42

Which classification group typically exhibits the highest electronegativity and is highly reactive in gaining electrons?

Alkali Metals Halogens (Group 17) Noble Gases (Group 18) Inner Transition Metals

43

Valence electrons are defined as the electrons located in the:

Innermost occupied energy level Nucleus of the atom Highest (outermost) occupied energy level Total number of $d$ and $f$ sublevels

44

The maximum number of electrons that can occupy the second main energy level ($n=2$) is:

2 8 18 32

45

As you move from left to right across a period, how does the number of valence electrons change (for main group elements)?

It remains constant It decreases steadily It increases steadily from 1 to 8 It increases then decreases

46

An element has an electron configuration of 2, 8, 3. Which group and period does this element belong to?

Group 3, Period 2 Group 13, Period 3 Group 3, Period 3 Group 13, Period 2

47

If an atom has 6 valence electrons, it is most likely located in which main group?

Group 6 Group 16 (Chalcogens) Group 14 (Carbon Group) Group 2 (Alkaline Earth Metals)

48

Elements in the same group have similar chemical properties primarily because they have the same:

Atomic radius Number of protons Number of core electrons Number of valence electrons

49

Why did Mendeleev have to leave gaps in his original table when arranging elements by atomic mass?

He believed those spaces were placeholders for the transition metals. He found that if he didn't leave gaps, elements would not align with others having similar chemical properties. He was waiting for accurate mass measurements for known elements. The noble gases were not yet discovered.

50

Consider Chlorine ($ ext{Cl}$). It is located in Period 3, Group 17. Based on its location and general properties, Chlorine is classified as a:

Metal Metalloid Noble Gas Nonmetal

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