C. Explain these atomic/ionic size differences: Na > CI Na > Nat Cl> CI
Which of the lists of increasing ionic radii is not correct? A) CI- < Br</ B) A13+ < Mg2+ < Nat C) Ca2+ < Sr2+ < Ba2+ D) S2- < Cl- <Kt E) Na* <02- <N3- ОА OB Ос OD OE
ULF C. Explain the reasons behind these 'atomic/ionic size differences: (15) i) atoms decrease in radius across a period ii) Group Il cations are smaller than the parent atom iii) anions are larger than the parent atom
Arrange these ions in order of increasing ionic radius: K+ .p3-, s2-, Cl-. O Cl- <52- <K+ <p3- O K+ < p3- < 52- <CI- O p3- < 52- < CI- <K+ O K+ < Cl- < 52- < P3- O cl- < 52- < P3- <K+
Select the correct statements about atomic and ionic sizes below. Check all that apply. O sis smaller than O Au is smaller than Au AP is smaller than Mg2 Na is smaller than Na Mg is smaller than Al Cl is smaller than CI CI is smaller than Cl Oo2 is smaller than S2 Au is smaller than Au Na is smaller than Na
Consider the following information for sodium and chlorine: Atomic radius: Na (186 pm) and Cl (100pm) Ionic radius: Na+(102pm) and Cl-(181pm) Why does the atomic radius decrease while ionic radius increase? The outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. Monatomic ions are bigger than the atoms from which they are formed. The outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. The...
Which of the following pair of elements/ions has a larger atomic/ionic radius? Explain (F,Br) (Al3+, Na+)
QUESTION 7 List the elements Na, Ca, Rb, CI, He in order of decreasing first ionization energy. He > C1 > Ca> Na > Rb He > Na > Ca> C1 > Rb Rb > Ca> C1 > Na > He He > Na> C1 > Ca > Rb
Quiz 4 Periodic Trends 1. Atomic and ionic radius trends. Circle ONE atom or ion from EACH pair that has the larger radius of the two. A. P or As B. Clor Cl C. Na or Mg D. Cr or Cr E. Br or Se 2. Isoelectronic pairs. Which of the following pairs is isoelectronic. Report the letter (A, B, C, etc) of your answer in the space beside the question number. A. P and As B. Cl and CI...
Give the formula for an ionic compound formed from each pair of ions. Na+ and 02- Na" and o> Ar* and FC A13+ and F- Mg2+ and S2- Ca2+ and P3-
The density of a NaCI crystal is 2.17 g/cm^3. The atomic mass of Na and Cl are 22 990 and 35.453 g/mole, respectively Compute the atom densities (in atoms/cm^3) of Na and Cl in the crystal.