Write the full electron configuration of the Period 2 element with the following successive IEs (in kJ/mol): IE1 = 801 IE2= 2427 IE3 = 3659 IE4= 25,022 IE5 = 32,822

Group the electronic configurations of neutral elements in sets according to those you would expect to show similar chemical properties. 1s²2s²2p63s²3p6 1s²2s²2p²³: Set A 1s²2s²2p 3s²3pº: 1s²2s²2p³ 1s²2s²2p 3s ²3 pº 4s²3d¹⁰4p⁰: 1s²2s²2p 3s²3p³: Determine the chemical symbols for the neutral elements corresponding to the electronic configurations. Use proper formatting; letter case matters. Answer Bank 1s²2s²2p 3s²3 p4s²3d¹04p6 1s²2s²2p 3s²3p³ Set B

F and F are both stable ions. What does this imply about the signs of the first ionization energy (IE₁) and electron affinity (EA) of F? IE₁ (F) 0, EA(F) > 0 IE₁ (F) = 0, EA(F) > 0 IE₁ (F) > 0, EA(F) 0

The graph below represents successive ionization energies (IEs) in kJ/mol for a particular element in period 3. Identify the element. 35000 30000 ll 25000 20000 15000 10000 5000 IE1 IE2 IE3 IE4 IES IE6 E7 E8 O Chlorine O Aluminum O Phosphorous Silicon O Argon Oxygen

Since the first ionization energy of rubidium is +403 kJ mol, how many kJ of energy is it required to convert 22.90 g gaseous rubidium to +1 monoatomic ion at constant temperature?

What element forms an ion with an electronic configuration of 1s2s²2p°3s²3p°4: 04p°5s²4d105p° (or [Xe]) and a -2 charge? Give the symbol for the element. element symbol:

Which group in the periodic table contains elements with the valence electron configuration of ns2np5?

element X has an electron affinity of 295.3 kJ/mol and the following ionization energies (in kJ/mol): IE1 = 1.008e3, IE2 = 1.846e3, IE3 = 3.20e3. In what column of the periodic table is this element probably found?

Which of the following statements are correct? o It takes a larger amount of energy to ionize a neutral, isolated, atom of an element with a ns?np? valence shell than to ionize an a neutral, isolated, atom of an element with a ns?np3 valence shell. The second ionization energy of an element with an ns' valence shell is smaller than the second ionization energy of an element with an ns? valence shell. The size of a cation is always smaller than the size of the corresponding neutral atom. The energy of a halogen atom in the gas state is smaller in magnitude than the energy of the corresponding halide anion in the gas state.

5) Give the name and symbols for three ions that are isoelectronic with an unknown element whose electron configuration is [ Kr] 5s², 4d¹0, 5p6. 6) Give the box orbital diagram for the ground state configuration of barium. 7) Give the name and symbols for two ions that are isoelectronic with selenium ion. 8) Find the possible values for the quantum numbers of the highest energy electron meaning that outermost valence electron. a. Gallium b. Rubidium c. Sodium