(a)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (a) with ‘
(b)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (b) with ‘
(c)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (c) with ‘
(d)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (d) with ‘
(e)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (e) with ‘
(f)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To Know the reactivity of an element (f) with ‘
(g)
Interpretation: The given electronic configurations of the elements have to be grouped, that represent elements with similar properties
Concept Introduction: In the periodic table the elements are grouped based on their valence electrons, so all the elements within a certain group have similar properties. Since only the valence electrons involve in bonding, reactivity of an element depends on the number of electrons present in the valence shell of the atom.
To group the properties of the elements with given electron configuration
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Chemistry: Atoms First
- Chemists can identify the composition of some unknown salts by conducting a flame test. Whenpotassium salts are heated in a flame, a purple color is observed. This is due to the movement ofelectrons between energy levels. What is the electron configuration of a potassium atom at groundstate?(A) 1s22s22p63s23p64d1(B) 1s22s22p63s23p63d1(C) 1s22s22d63s23d64s1(D) 1s22s22p63s23p64s1arrow_forward10. Identify the elements (two of these are irregular, so pay close attention).(a) 1s22s22p63s23p64s23d104p65s24d5 (b) [Xe]6s24f145d106p5(c) 1s22s22p63s23p64s23d104p65s24d105p66s14f145d10 (d) [Rn]7s25f76d1arrow_forward(1) What is the valence electron configuration for the helium atom? (2) What is the valence electron configuration for the gallium atom? (1) What is the name of the element with a valence electron configuration of 3s23p2?(2) What is the name of the element with a valence electron configuration of 4s1?arrow_forward
- (1) What is the element with an electron configuration of 1s22s22p63s23p64s23d3?fill in the blank 1(2) What is the element with an electron configuration of 1s22s22p63s23p64s2?fill in the blank 2arrow_forwardWhat element has the ground state electronic configuration [Ne]3s? (A)Na (B)Mg (C)F (D)Ca (E)Karrow_forward. (2) Which of the following electron configurations corresponds to the ground state of anatom of an alkaline earth metal element?1s22s22p5 1s22s22p63s23p64s23d104p2 1s22s22p63s23p64s23d104p65s11s22s22p63s23p64s23d7 1s22s22p63s23p64s2 1s22s22p63s23p1arrow_forward
- (D) Z 22. Valence electrons in an atom of phosphorus are closer to the nucleus than the valence electrons of aluminum because: (A) P has a greater effective nuclear charge and a greater shielding than Al. (B) P has a greater effective nuclear charge with the same shielding as Al. (C) P has the same effective nuclear charge with greater shielding than AI. (D) P has the same effective nuclear charge and the same shielding as Al. Education TM, Inc. DELL F2 F3 F4 F5 F6 F7 F8 F9 # 2$ & 8) 2 3 4 6. 7 80 W E T Y F Garrow_forward21. The chart below shows the relationship between ionization energy and the increase in atomic number. The letter on the chart for the noble gases (Group 18) is most likely: W Alomic number increases (A) W (B) X (C) Y (D) Z 22. Valence electrons in an atom of phosphorus are closer to the nucleus than the valence electrons of aluminum because: (A) P has a greater effective nuclear charge and a greater shielding than Al. (B) P has a greater effective nuclear charge with the same shielding as Al, (C) P has the same effective nuclear charge with greater shielding than AI. (D) P has the same effective nuclear charge and the same shielding as Al. increasesarrow_forwardWhich element in each of the following sets would you ex-pect to have the highest IE₂?(a) Na, Mg, Al(b) Na, K, Fe(c) Sc, Be, Mgarrow_forward
- Portions of orbital diagrams representing the ground-state electron configurations of certain elements are shown here: ↑ ↑ ↑ ↑ ↑ ↑ ↓ ↓ ↑ ↑ ↓ ↑ (a) (b) (c) ↑ ↓ ↑ ↑ ↑ ↑ ↑ ↑ ↓ ↑ ↓ (d) (e) ↑ ↓ ↑ ↓ ↓ ↓ ↑ ↓ ↑ ↓ (f) Which violate the Pauli exclusion principle? a b c d e f Which violate Hund's rule? a b c d e farrow_forwardWhat is the electron configuration for Tellurium (Te)? A) 1s²2s²2p 3s²3p 4s²3d¹04p4 B) 1s²2s22p 3s²3p 4s²3d¹0 4p5s 5p4 C) [Kr] 5s²4d¹05p4 2 D) 1s²2s²2p 38² 3p 4823d¹04p6 58² 4d¹0 5p4 E) [Kr] 58² 4d¹03f¹5p¹ O O B O B and E O A E B and C A and Darrow_forward(1) What is the name of the element with a valence electron configuration of 2s22p3?fill in the blank 1(2) What is the name of the element with a valence electron configuration of 3s2?arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning