8.2 Use the second member of each group from Group 1A to Group 7A to show that the number of valence electrons on an atom of the element is the same as its group number.

Q: Consider the isoelectronic series Zr4+, Nb5+, Mo6+, Tc7+. Arrange these species as follows. (Use the…

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Q: Arrange each of the following sets of atoms and ions, inorder of increasing size: (a) Se2-, Te2-,…

A: The Atomic and Ionic size increases from top to bottom in the group with the increases in number of…

Q: (a) Use orbital diagrams to illustrate what happens when anoxygen atom gains two electrons. (b) Why…

A: The effect of gain of two electrons by oxygen atom is to be illustrated using orbital diagram. Why…

Q: Use the second member of each group from Group IA to Group 7A to show that the number of valence…

A: Group 1A Second element is Na (Z = 11) Electronic configuration 1s2 2s2 2p6 3s1 Group 2A Second…

Q: Which of the following series is isoelectronic? O a. H, He*, Li2+, Be3+ O b. 02-, 1", Ar, Na*, Mg²+…

A: The species which have the same number of electrons are isoelectronic to each-other.

Q: In the isoelectronic series Ca2+, Cs+ , Y3+ , state which ion is largest?

A: Among Ca2+, Cs+ , Y3+ the largest ion will be:

Q: Describe the periodic trends in radii?

A: Atomic radii increases as we move down the group because effective nuclear charge decreases. So…

Q: Which halogen has the highest ionization energy? Explain why.

A: Hi, since you have posted multiple questions. We will answer the first questions. Kindly repost the…

Q: Arrange these ions from largest to smallest ionic radius Ba2+,  Cs+,  Te2-,  I,  Sb3-

A: ions from largest to smallest ionic radius is  Sb3- >Te2- >  I  >  Cs+  > Ba2+

Q: Explain the relationship between the properties of an elementand the number of valence electrons…

A: Valence electrons are the total number of electrons present in the outermost orbital of an atom.…

Q: Which atom and/or ion is (are) isoelectronic with Bromide anion (Br-)? List all that apply Se2-,…

A: Isoelectronic species are those species which contains equal number of electrons. Br- contains 36…

Q: 7.109 Write the formulas and names of the hydrides of thefollowing second-period elements: Li, C, N,…

A: The name and formula of hydrides of the elements have to be predicted. Their reactions with water…

Q: Which element, W or Au, has the greater number of electrons in antibondingorbitals?

A: Atomic number of tungsten (W) is 74 and atomic number of Gold (Au) is 79. So, Au has more electrons…

Q: Arrange the following isoelectronic series in order of increasing atomic radius: Se?-, Sr2+, As³-,…

A: Given  isoelectronic Species = Se2- , Sr2+ , As3- , Rb+ , Br-  Increasing order of atomic Radius =

Q: Discuss the importance of electron affinity and ionizationenergy in the formation of ions.

A: Electron affinity:   release of certain amount of energy when an electron is added to neutral…

Q: #9 Which group d has the lowest element ionization energy A) Bi) Ne c) Be Pi) Ra Li

A: Since you have posted multiple questions and asked the only 9th question, we will solve the 9th…

Q: Arrange the following in order of increasing radius and increasing ionization energy. a. N+,N,N- b.…

A: Ionization energy: The amount of energy required to remove a valence electron from an isolated…

Q: 7.5 B List all the common ions that are isoelectronic with Ne.

A: Isoelectronic species are those species which have same number of electrons. For example - Neon (Ne)…

Q: Which of the following is an isoelectronic series? 1. B5, Srª“, As³-, Te?- II. F', Cl', Br", I" III.…

A: In isoelectronic species, all the species have same number of electrons.

Q: WHAT IS THE ELEMENT: a) of Group 4A, with the most metallic character b) of Group 5A which forms the…

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Q: Write the electron-dot symbol for any element X in group 3A.

A: Lewis structure represents the valence shell electrons in a compound. It shows the distribution of…

Q: 3. Arrange the following groups of atoms/1ons in order of increasing size.

A: Atomic size is the distance between the centre of the nucleus of an atom and its outermost shell…

Q: A group of species is given to you: ci', Kr, Ne, Ar, P³,s“ and K". Identify the species that are…

A: Isoelectronic species are those species which have same number of electrons present in it. The given…

Q: 6. From the Periodic table, choose 2 metals from the Alkaline metal series, 2 metals from the…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: The last orbital of element Y’s electronic configuration is defined by the following set of quantum…

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Q: Without consulting any tables, arrange the following sub- stances in order and explain your choice…

A: Since you have posted multiple questions, we will solve only first question for you. To get the…

Q: Arrange the following cations in order of increasing ionic radii: Fr+, Cs+, Rb+, B3+, Al3+, Ga3+

A: Arrange the following cations in order of increasing ionic radii: Fr+, Cs+, Rb+, B3+, Al3+, Ga3+

Q: a) Which element is least likely to lose an electron? Choose one: He, Be, Na, Mg, Ca, Sr, b) Why…

A: a) The element which is least likely to lose an electron has to be identified b) The reason why the…

Q: 1

A: Dear student I have given answer to your question in the image format.

Q: Order each of the following sets of five atoms and ions according to increasing size. ("1" smallest…

A: The order of the size of the elements according to increasing size is given below

Q: Arrange the following in order of increasing first ionization energy: B, O, N, C, F

A: The minimum energy required to release the most loosely bound electron from the valence shell of a…

Q: Arrange the following elements in order of decreasing atomic radius: Cs, Sb, Cl, Pb, As. Rank…

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Q: 11) Which of the following is an isoelectronic series? A) 02-, F, Ne, Na+ B) S, a, Ar, K E) Si2-,…

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Q: The first three ionization energies of an element X are 590, 1145, and 4912 kJ/mol.  What is the…

A: Ionization energy is the energy required to remove an electron from its atom in gaseous state. 1st…

Q: A – most electronegative element in - Period 4. B - smallest atom in Group 5A. C- alkaline earth…

A: A - most electronegative element in Period 4. Answer : bromine Reason : the tendency to attract…

Q: Consider the elements selenium (Se) and bromine (Br). Whichhas the higher first ionization energy?…

A: From the given two elements which has higher first ionization energy and higher electron affinity…

Q: Why does potassium have a lower first ionization than lithium ?

A: Electronic configuration of Li : 2,1 Electronic configuration of K : 2,8,8,1

Q: Explain why electron affinity increases across a period and decreases down a group

A: Electron affinity -it is the amount of energy released when an electron is added to a neutral atom…

Q: What is the electron configuration of the element in the 4th period of Group 5A (IUPAC Group 15),…

A: Using a periodic table, we can identify the element in the 4th period of Group 5A. The element in…

Q: How many electrons does barium have to give up to hav the same electron configuration as a noble…

A: The electron configuration of an atom is the representation of the arrangement of electrons…

Q: Why is the ionization largest at the end of a period, but drops drastically at the start of the next…

A: Energy needed for removal of an electron from isolated gaseous atom is known as ionization energy.

Q: Explain why ionization energy increases across a period and decreases down a group.

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Q: Arrange the following in order of increasing radius and increasing ionization energy.a. N+, N, N-b.…

A: Ionization energy: The amount of energy required to remove a valence electron from an isolated…

Quantum Chemistry

Quantum chemistry deals with the properties of chemical systems and their reactions. The branch of chemistry which is more concerned with quantum chemistry is physical chemistry. It is a more sophisticated field of theoretical physics which is concerned towards the application of physical concepts towards various chemical aspects such as, formation of atoms, chemical structure descriptions, chemical bond strength, hybridization, conjugation etc. Quantum chemistry mainly studies the various states i.e., ground state, excited state, transition states of the individual atoms or molecules taking place during any chemical reaction. The laws of motion explained by various scientists, which are termed as “classical mechanics” were not acceptable in terms of electrons, protons, atoms, light etc. Thus, a new theory named “quantum mechanics” emerged to understand the basic framework of various atomic and subatomic particles.