Element X is Iodine as it has the highest first electron affinity
Element Y is Barium
Barium is the second largest element in its period and has valence electrons in n=6 .
Most stable compound formed would be BaI2
Element x has the highest first electron affinity in its period, the ground state electron configuration of its common is: [Kr] 5s2 4d10 5p6 Element Y is the second largest element in its period; its valence electron are in
Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. If the configuration is a noble gas, enter the noble gas in
Identify the neutral element represented by this excited-state electron configuration, then write the ground-state electron configuration for that element. Excited State: 1s2 2s2 2p2 3s1 Element Symbol: ? Ground State: ?
Consider the following neutral electron configurations in which 'n' has a constant value. Which configuration would belong to the element with the most negative electron affinity, E-ea? a) ns^2 b) ns^2 np^2 c) ns^2 np^5 d) ns^2
Hi! Can somebody please help me with a coupla questions? Thanks loads!!! Describe physical and chemical properties of isotopes of the same element. Given the electron configuration of an element, how can you tell whether it
If you maximize the unshared electrons in the boron atom, the electron configuration is? i know the electron configuration at ground state is 1S2 2S2 2P1 but when it maximizes unshared electrons i don't understand how it affects
I need to know the predicted and actual electron configuration for Lanthanum I know for lets say Cr the predicted config is [Ar] 3d44s2 and the actual is [Ar]3d54s1 but lanthanum is different and i don't know how to do it. Any