what are the two quantum isonomers comprising the atomic nucleus in [Pt(NH3)4(Cl)2]Cl2 ?
401509
I don't know that question.\n\nI can tell you that it's an octahedral complex. The two isomers would be CIS (Both chlorides adjacent to each other) and TRANS (both chlorines opposite each other)
57944
Name: Chlorine \nSymbol: Cl \nAtomic Number: 17 \nAtomic Mass: 35.4527 amu \nMelting Point: -100.98 °C (172.17 K, -149.764 °F) \nBoiling Point: -34.6 °C (238.55 K, -30.279997 °F) \nNumber of Protons/Electrons: 17 \nNumber of Neutrons: 18 \nClassification: Halogen \nCrystal Structure: Orthorhombic \nDensity @ 293 K: 3.214 g/cm3 \nColor: green
962694
Tehe answer is:\nAg + HNO3 -> AgNO3 + H\nAgNO3 + KBr -> AgBr + KNO3
980851
C, having both positive and negative charges on one molecule.
64389
Platinum chloride should be soluble and dissociate into Pt4+ (platinum (IV))and Cl- (chloride) ions.
17774
It doesn't give me room to list them all and explain them on here so let me direct you to a website I found that does a pretty good job:\nhttp://vergil.chemistry.gatech.edu/notes/quantrev/node20.html
72779
A molecule is made up of atoms.
913568
Zn(NO2)2; Co(HSO3)3; HgF; Al2(CO3)3; Cs2C2O4; Ba(ClO)2; SnBr2; Mg(HSO3)2.
127454
If such a compound existed, it would be ionic. Calcium (IV) Chloride.\n\nBut it won't exist, particularly as an ionic compound. You're not going to be able to pull the p electrons from the calcium without a fight and chlorine isn't strong enough (or even fluorine, for that matter). Maybe you can achieve the species in the gas phase ... I don't know.\n\nIf it's covalent, what possible structure could it have? What do the bonding orbitals look like?
797121
The answers are KCl, CaF2, and Na2O. Potassium has one electron on the outer ring while chlorine has seven. To make chlorine's ring "full" potassium gives the one electron to chlorine. They are "happy" now. :) That's what my science teacher told me. He's weird.
603078
a) Ru - ruthenium\nb) S - sulfur\nc) Ir - iridium; with an incomplete d-subshell, it must be a transition metal\nd) Sb - antimony
98695
My answer is,\n \nNH4NO3(ag) + KOH(aq) -> NH4OH(aq) + KNO3(aq)
525984
Diatomic molecules contains two atoms (either same atoms or two different). Examples are, H2, O2, N2, Cl2, CO, NO etc.
613727
try:\nhttp://lb.chemie.uni-hamburg.de/static/data/50_zzk46n8n.html
825051
Covalent bonds, as in NH4+
867434
Construct a Lewis structure for NH3 ( Use N as the central atom ):  first: Determine the total number of valence electrons in the molecule.  In this case there are 8.  Represent shared pairs of electrons between the bonded atoms.  There will be one line connecting each atom, with each line representing two electrons, accounding for six of the eight available electrons.  With the remaining two valence electrons, position them on the fourth unbonded side, satisfying the octet rule for Nitrogen.\n\nThe above described Lewis structure gives you the molecular structureTrigonal Pyramidal ( three bonding pairs and one non bonding pair)\n\nRules for predicting molecular shape by VSPER theory:\n\n1.  Determine Lewis structure\n2.  Determine the number of electron pairs (bonded and non bonded) surrounding a central atom.\n3.  Use VSEPR theory to decide what symmetrical three dimensional shape will accommodate all bonded and non bonded electron pairs.\n4.  Classify the shape of the molecule by considering the arrangement of the joined atoms only, ignoring the nonbonded electron pairs.  That is why, although the NH3 molecule  has four pairs of electrons around the central atom, ammonia's shape is trigonal pyramidal.
904363
(NH4)2CO3+MgSO4->(NH4)2SO4+MgCO3