For each of the following pairs, indicate which element hasthe smaller first ionization energy: (a) Ti, Ba; (b) Ag, Cu;(c) Ge, Cl; (d) Pb, Sb.
Q: Which of the following sets of quantum numbers would account for the highest-energy electron in…
A: The highest energy electron in Ni2+ ion corresponds to a certain set of quantum numbers. The…
Q: Why are the ionization energies of the alkali metals in the order Li >, Na > K > Rb?
A: ANSWER IS DISCUSSED BELOW :
Q: Platinum hexafluoride, PtF6 has a very high electron affinity (772 kJ/mol) but when lithium metal is…
A: Lithium has a very small size and has the maximum polarizing power due to its small radius.
Q: 22. Order the following isoelectronic species by increasing ionic radius: Cl¯, Ar, and P³-.
A: For isoelectronic species , more it accept electrons then more its size.
Q: The first element of every group behaves differently from the other elements in the same group.…
A: Lithium shows anomalous behavior because it has the smallest size in the group. Since it has the…
Q: Predict the trend in values of Slater's constant of the every first element of each group of p…
A:
Q: Which atom has the same electron configuration as In? In3+? Ga Zn Pd Ir O Te
A: The element having same number of electrons as In3+ will have same electron configuration as In3+
Q: (a) Does metallic character increase, decrease, or remainunchanged as one goes from left to right…
A: (a) Metals forms cation by the loss of electrons. On going across the period in the periodic table,…
Q: Write the balanced chemical equation for the reaction of scandium oxide with nitric acid?
A: The given reactants are Scandium oxide and Nitric acid.
Q: 7.119 The first four ionization energies of an element areapproximately 738, 1450, 7.7 × 103 , and…
A: The first four ionization energies of an element are approximately 738, 1450, 7.7 × 103, and 1.1 ×…
Q: Q.Arrange the following in their increasing size with the help of slater’s rule and also give…
A:
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: Despite the expected decrease in atomic size, there is an unexpected drop in IE1 values between…
A: Ionization enthalpy, IE, is also called ionization potential is the ability to remove the electron…
Q: How many unpaired electrons would be present on a Be2 2− ion? Would it be paramagnetic or…
A: On Be2 2- ion,there will be two unpaired electrons in the molecular orbitals.As there are two…
Q: How does the variation in atomic size across a transition se-ries contrast with the change across…
A: The transition elements are those elements in which the last electron enters the d sub-shell. The…
Q: Which element has the highest second ionization energy: Li,K, or Be?
A:
Q: Which should have the largest difference between the first and с. second ionization energy-C, Li, N,…
A: (c) Given atoms are - Carbon C , Lithium Li, Nitrogen N, Beryllium Be Carbon has total 6…
Q: Consider the isoelectronic ions Cl- and K+. (a) Which ionis smaller? (b) Using Equation 7.1 and…
A: (a)
Q: Which of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest? Which of the elements of…
A:
Q: An atom of which of the following elements has the smallest first ionization energy? Rb or Si or F…
A: The energy which is needed to remove an electron that is loosely attached to an isolated gaseous…
Q: Which element, indicated by letter on the periodic table above, has a 2+ ion with the electron…
A:
Q: Describe how to write an electron configuration for a transition metal cation. Is the order of…
A: The electron configuration of a transition metal cation is written by removing the electrons first…
Q: it is clear that the first ionization energy of He is very large. Would you expect the first…
A: We have helium and H-( Hydride ion) H- has lower first ionisation energy than He.
Q: (ii) Lithium shows a diagonal relationship with magnesium, A) Why are these elements diagonally…
A: A.Following are the main reason of diagonal relationship shown by Li and Mg.
Q: Explain the theoretical aspect of the separation of Group IIA cations from Group IIB.
A: Cations of group II are known as Copper arsenic group in qualitative analysis. This group II has…
Q: Question attached
A: Given,
Q: The orbital occupancies for the d orbitals of several com-plex ions are diagrammed below. (a) Which…
A: Since you have posted the multiple part subpart question we are supposed to answer three subparts.…
Q: Which of the halogen elements has the highest density in its standard state? B) Which of the…
A:
Q: Which of the following does have the highest ionization energy? ? Z of Mg =12, K =19, Na = 11, Cl…
A: Ionization energy is defined as the amount of energy required to remove the most loosely bound…
Q: (a) What trends, if any, exist for Z(eff )across a period and downa group? (b) How does Z(eff)…
A: Z(eff) is the net attractive force exerted by the nucleus on the valence electrons.
Q: Why is sodium (Z = 1 1) the next univalent atom after lithium
A: We know univalent atom present in the group 1. And group 1 contain H,Li,Na,K,Rb,Cs,Fr The…
Q: What is the relationship between the value for the first ionization energy of a Cl-1g2ion and the…
A: Ionization energy is defined as the amount of energy that is required to remove an electron from a…
Q: Which is smaller, S2- or Ca2" ? Which is more reactive, Cs or Sr? 9. Write the reaction equation…
A: Given: S2- and Ca2+
Q: Consider the elements: Na, Mg, Al, Si, P.a. Which element has the highest second ionization…
A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…
Q: A. If an element with the valence configuration 4s'3d10 loses 2 electron(s), these electron(s) would…
A: Element first looses electron from outermost shell and then from the n-1 shell Element accepts…
Q: Arrange the following elements in order of decreasing atomic radius: Cs, Sb, Cl, Pb, As. Rank…
A:
Q: Which element will display an unusually large jump in ionization energy values between I3 and l4,…
A: Ionization energy is the amount of energy required to remove an electron from an isolated atom or…
Q: As we move across a period of the periodic table, why dothe sizes of the transition elements change…
A: The reason is as given below;
Q: Write any two multiplicities of higher energy in the form 2s+1L J, giving a diagrammatic…
A: The term 2s+1L is an atomic term where, S is the total spin angular momentum for each individual…
Q: 0OMEA Ot the elements below iS Smaller than Ca but larger than As ? Br P Mn what is the valence…
A: Using concept of periodic properties of elements.
Q: Which of the following has the highest electron affinity? F, Si, P or S.
A: Electron affinity is the amount of energy released when an extra electron is added to the neutral…
Q: What element is the electron configuration for Cl- isoelectric with?
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Which element would you expect to be more metallic?(a) S or Cl(b) In or Al(c) As or Br
A: Metallic character represents the tendency of element to behave as metal. It increases in a group…
Q: 3. Which one of each of the following pairs has the higher electron affinity? Explain in detail for…
A: We have to select each of the element whic greater electron affinity from the given following…
Q: Which element had the smallest ionization energy , He , Ar , Xe
A: Ionization Energy (I.E.)- Amount of energy required to remove last shell electron of an isolated…
Q: Among the period 4 transition metals (Sc–Zn), which elements do not form ions where there are…
A: The transition element present in the fourth period are Scandium, titanium, vanadium, chromium,…
Q: In each of the following sets, choose the one with the highest ionization energy а. К, К", Са, Са*?…
A: Those compound which have nobel gas electronic configuration ,have high ionisation energy
Q: 8. Put in order of decreasing atomic radii (largest to smallest): CI, As, S Put in order of…
A:
For each of the following pairs, indicate which element has
the smaller first ionization energy: (a) Ti, Ba; (b) Ag, Cu;
(c) Ge, Cl; (d) Pb, Sb.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- Using only the periodic table, arrange each set of atoms inorder from largest to smallest: (a) K, Li, Cs; (b) Pb, Sn, Si; (c) F,O, N.7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°When a nonmetal oxide reacts with water, it forms anoxoacid with the same nonmetal oxidation state. Give the name and formula of the oxide used to prepare each of these oxoacids:(a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitricacid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.
- 6. Arrange the following chemical species in order of increasing atomic radius. Explainyour arrangement in each case.(a) K, Mg, Ca, Aℓ(b) F–, S2–, Cℓ–.Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheresbelow represent these four ions, scaled according to ionic size.(a) Without referring to Figure 7.8, match each ion to its appropriatesphere. (b) In terms of size, between which of the sphereswould you find the (i) Ca2+ and (ii) S2- ions?la) For each of the following pairs indicate which element you would expect to have the larger First Ionization Energy and which one would have the larger radius: (a) Ca and Cl; (b) Sn and Tl; (c) Ba and Bi (d) Fr and Cs b) For each pair indicate which Ion you would expect to have the largest Radius: (a) 0²- and O; (b) N³ and Mg²+ (c) Al3* and Al ne Ele
- Arrange the following chemical species in order of increasing atomic radius. Explain your arrangement in each case. (a) K, Mg, Ca, Al (b) F–, S2–, Cl–.Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?10. Which of the following element has paramagnetic property? (a) Mg (b) P (c) Ne (d) Hg 11. Which of the following element is a main group (representative group) element? (a) Zn (b) S (c) Cu (d) Co 12. The energy required to remove an electron from an atom in its ground state is called (a) atomic number (b) electronegativity (c) electron affinity (d) ionization energy
- When a nonmetal oxide reacts with water, it forms an oxoacid with the same oxidation number as the nonmetal. Give the name and formula of the oxide used to prepare each of these oxoacids: (a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitric acid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.8.37 On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs: (a) Na, Cs; (b) Be, Ba; (c) N, Sb; (d) F, Br; (e) Ne, Xe.The elements of a period in the periodic table are given below in order from left to right: 3Li 4Be 5B 6C 80 (1) To which period do these elements belong? (11) Which of them will have the largest atomic radius. Explain the trend.