Answer true or false. (a) Elements in the same column of the...

Answer true or false. (a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration. (b) All Group 1A elements have one electron in their valence shell. (c) All Group 6 A elements have six electrons in their valence shell. (d) All Group $8 \mathrm{A}$ elements have eight electrons in their valence shell. (e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth. (f) Period 2 results from filling the 2s and 2 $p$ orbitals, and therefore, there are eight elements in period 2. (g) Period 3 results from filling the 3s, 3p, and 3d orbitals, and therefore, there are nine elements in period 3. (h) The main-group elements are $s$ block and $p$ block elements.

Answer true or false.
(a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration.
(b) All Group 1A elements have one electron in their valence shell.
(c) All Group 6 A elements have six electrons in their valence shell.
(d) All Group $8 \mathrm{A}$ elements have eight electrons in their valence shell.
(e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth.
(f) Period 2 results from filling the 2s and 2 $p$ orbitals, and therefore, there are eight elements in period 2.
(g) Period 3 results from filling the 3s, 3p, and 3d orbitals, and therefore, there are nine elements in period 3.
(h) The main-group elements are $s$ block and $p$ block elements.

Key Concepts

Periodic Table Structure

The periodic table is organized into rows (periods) and columns (groups). Elements within the same group often display similar chemical and physical properties because they typically have the same number of valence electrons. This structure helps in predicting patterns and trends among elements.

Electron Configuration

Electron configuration describes how electrons are distributed in atomic orbitals. The outer-shell (valence) electrons are particularly important because they determine an element's chemical reactivity. Elements that have similar electron configurations in their outer shells often exhibit similar chemical properties.

Orbital Filling Order

The order in which electron orbitals are filled (based on the Aufbau principle) determines the number of electrons that can be accommodated in each period. This explains why certain periods can hold a specific number of elements, corresponding to the filling of different orbitals such as s, p, d, and f.

Valence Electrons

Valence electrons, which are the electrons in the outermost shell of an atom, largely determine an element's chemical behavior and bonding properties. In main-group elements, the number of valence electrons is closely tied to the group number, affecting their placement in the periodic table and their reactivity.

Blocks in the Periodic Table

The periodic table is divided into blocks (s, p, d, and f) based on the type of atomic orbital being filled by the electrons. The main-group elements are primarily found in the s and p blocks, where their predictable electron configurations help explain periodic trends in properties and reactivity.

Transcript

00:04 Hey guys, let's do problem 54.

00:06 In this problem, pv statements are given.

00:09 We need to figure out if these statements are true or false.

00:14 The first statement is that elements in the same column of the periodic table have the same outer shell electron configuration.

00:22 The same column elements in the same column means each of these columns they belong to certain group.

00:28 The first column here it is group 1a then second column is 2a here we see group 3a 4 a 5a 6a and finally 8a these are the same columns belong to our same group now we know that for main group elements main group elements means the elements that belong to this a groups for main group elements the number of valence electrons this corresponds to the group number it means that group number is the same column so for group a elements the number of valence electrons now valence electrons are the outer most shell electron therefore for group a elements the number of valence electrons corresponds to the this corresponds to the group number now elements with the same balance electrons are placed in the same groups.

01:52 That is what it means.

01:54 Therefore, the elements placed in the same column or group of this table have the same outer shell electron configuration.

02:06 The elements placed in the same column or group of the periodic table have the same outer shell electron configuration.

02:33 Therefore, we can say that this is a true statement.

02:43 And we can, excuse me, we can also check the electron configuration for the same group elements.

02:50 For example, we can check that for one group 1 element, lithium, which is having the atomic number of 3 and sodium, which is having the atomic number of 11.

03:04 The electron configuration for lithium is 1s2, 2p1.

03:09 1 s2 s 1 and for sodium that is 1 s 2 2 s 2 2 p 6 3 s 1 therefore we see that the elements of the same period which is the same column which is group 1a of this period table they are having the same outer shell electron configuration the outer shell number is changing to 3 but they are having only 1 electrons both of the outer sheds are having only one electrons.

03:44 Now we can move to the second statement.

03:47 All group 1a elements have one electron in their balance shell.

03:52 This is again a true statement.

03:56 In the periodic table elements with the same balance electrons they are placed in the same column or group.

04:02 Therefore all the elements with one electron in their outermost shell are placed in group 1a.

04:09 We can again check some electron configuration.

04:14 So we have hydrogen with only one electron.

04:17 The electron configuration is 1s1.

04:20 Therefore, it is going to hydrogen.

04:24 It is going to group 1a.

04:26 We have potassium with 19 atomic number.

04:30 Therefore, potassium is having 19 electrons.