Which of the following atoms is isoelectronic with Br-?
957155
It will be Kr because isoelectronic means having same number of electrons. As you have Br- so total electrons will be 36 (ie 35 for br and one of the gained electron ) . Ar has 18 elctrons, Kr has 36 electrons while Se has 34 electrons. so it will be Kr
87280
MBrO3-9H2O where M can be Na,K,Li, other +1 cations\n\nIf M is other than these you have to adjust subscripts
813911
HBr ---> H(+) + Br(-)\nH2SO3 ---> H(+) + HSO3(-)\nCH3-COOH ---> H(+) + CH3-COO(-)
1021348
1. Platinum-pt\n2. Boron-b+3\n3. Galium-ga+3\n4. Nitrogen-n-3\n5. Carbon-c\n6. Silicate-Si+4\n7. Fluorate-f-1\n8. Iodate-I-1\n9. Astatate\n10. and the ionic formulae for all of the transition elements that you kn\nget more here below
634552
an ion with both acidic and basic part
1172979
Lead II Nitride\n\nCa(BrO2)2
807050
B(OH)3\n\nThe following link has a neat picture of what the molecule could look like.
811889
No concrete way to work it out. Groups one and two take positive charges equal to their group number (Mg2+, Li1+ etc). Groups 3, 4, 5, 6 and 7 ionise to a negative charge of 8 minus their group number (Cl1-, O2- etc), though 3, 4, and 5 tend to resist ionisation and are much more commonly found bonded covalently. The Transition elements ion charges are virtually impossible to predict without an extensive knowledge of d orbitals etc..
961493
You need to know more than just the electron configuration.  There is contraction from left to right on the periodic table, plus additional periodic trends that must be considered.   \n\nEven more importantly, you need to define whether you are looking for the largest element IN ITS NATURAL  STATE (i.e. Cl2, Hg metal, etc) or AS THE ION.   Atomic and ionic radii differ.\n\nMore clarity is needed here.
337603
Here is the answer.. Just remember periodi table...\nElements on left most side are electro positive and elements on right most are electro negative. (The last row is nobel gases..so leave it)\nNow Cl- belongs to right most side... its more electro-ve\nRb, Ca are on left side.... they are electro positive(They will give  electron with out much force)\nSi, S are in middle-- their properties are in between...\n\nThats it!
732674
HBr is a strong acid because of Bromine's electronegativity.
556705
Ba(OH)2, MgBr2, CH3COOH, NH4OH\n\nFirst two are strong electrolytes, second two are weak (do not completely dissociate).
712728
choose the noble gas that comes before the element.   in Mn(2+)'s case, that's Ar\n\nwrite the noble gas down in brackets, and continue on with the electron config. as normal\n\n[Ar}4s23d3\n\nFor O(2-), it turns into Neon so it would just be [Ne]
802906
they fill the s orbitals with 2 electrons
832151
I think d). Br- can be a good leaving group and be displaced by an appropriate chemical (nucleophile).
813548
The answer is a) Krypton.\n\nThe bromide anion exists as Br-.\nWith the single negative charge, you know that it has an extra electron, therefore it's electron config is like the noble gas nearest to it on the periodic table: krypton.
1058444
Mg2+ < Na+ < Br-\n\nIon size depends first on the main quantum number. Na and Mg both strip down to the Ne configuration, while Br takes up the Xe configuration, two main quantum numbers higher.\n\nMg2+ is smaller than Na1+ because the remaining electrons are subject to a stronger electrostatic field.\n\nThe above is true for ions in crystal lattices.\n\nNote that in watery solutions ion size has to be calculated differently when you take the hydrate shell into account. Na+ becomes Na(H2O)6(1+), and Mg2+ becomes Mg(H2O)6(2+). Bromide won't take up a regular hydrate shell.