16. Select the correct statement below: Phosphorous contains 10 core electrons and 5 valence electrons. Its orbital diagram contains one half-filled 3p orbital and two filled 3p orbitals. Aluminum contains 10 core electrons and 3 valence electrons. Its orbital diagram contains three half-filled 3p orbitals. Calcium contains 18 core electrons and 2 valence electrons. Its orbital diagram contains two half-filled 4s orbitals and no filled 4p orbitals. Sodium contains 10 core electipns and 1 valence electron. Its orbital diagram contains one half-filled 3s orbital and three empty 3p orbitals. a) b) c) d)

16. Select the correct statement below: Phosphorous contains 10 core electrons and 5 valence electrons. Its orbital diagram contains one half-filled 3p orbital and two filled 3p orbitals. Aluminum contains 10 core electrons and 3 valence electrons. Its orbital diagram contains three half-filled 3p orbitals. Calcium contains 18 core electrons and 2 valence electrons. Its orbital diagram contains two half-filled 4s orbitals and no filled 4p orbitals. Sodium contains 10 core electipns and 1 valence electron. Its orbital diagram contains one half-filled 3s orbital and three empty 3p orbitals. a) b) c) d)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Order the following elements from largest atomic radius to smallest? Group of answer choices Ca > Ga > Se > Kr Kr > Se > Ga > Ca Ga > Ca > Se > Kr Kr > Ca > Ga > Se
15
Consider the main group elements of Period 3 in the periodic table: sodium (Na), magnesium (Mg), aluminum (Al), silicon (Si), phosphorus (P), sulfur (S), and chlorine (Cl). Arrange these elements in order of increasing atomic radius and explain the observed trend. b
11
PART C: ELECTRON CONFIGURATIONS Questions: C1. Write the full electron configurations for the following elements. Ве Na Mg Al Si CI Ar K Sc Ti Mn Fe Ni Zn Ga As Br Kr
4. Calcium has 20 electrons in total. The ionization energy for the first 18 have been graphed below. Provide appropriate labels for the two empty boxes. IONISATION ENERGY (kJ mol¹) 120000 100000 80000 60000 40000 20000 O IE3: REMOVAL OF ELECTRON FROM 3p 1 2 3 IE 17: REMOVAL OF ELECTRON FROM 2s 4 5 6 7 NUMBER OF ELECTRONS REMOVED 8 9 10 11 12 13 14 15 16 17 18
Predict the electron configuration for the C atom: Predict the electron configuration for the P atom: Predict the electron configuration for the V atom: Predict the electron configuration for the Sb atom: Predict the electron configuration for the Sm atom: Predict the electron configurations of N3– Predict the electron configurations of Ca2+ Predict the electron configurations of S2– Predict the electron configurations of Cs1+ Predict the electron configuration of Cr2+ Predict the electron configuration of Gd3+
Which statement is true about trends in metallic character? metallic character increases as you move to the right acrosss a row in the periodic table and increases as you move down a column metallic character increases as you move to the right across a row in the periodic table and decreases as you move down a column metallic character decreases as you move tot he right across a row in the periodic table and increases as you move down a column metallic character decreases as you move to the right across a row in the periodic table and decreases as you move down a column
Part A: How does ionization energy change down a group? increases from left to right decreases from left to right increases from top to bottom decreases from top to bottom Part B: Why is Ionization energy smaller for larger atoms? Sheilding. The nucleus cannot hold onto the electrons as well and loses them easier Shielding. The nucleus holds onto the electrons stronger and does not lose them easily There is no explanation Part C: According to the trend, which of these 4 elements has the largest ionization energy? Be (atomic# 4) Sr (atomic# 38) F (atomic# 9) I (atomic# 53) Part D: According to the trend, which of these 4 elements has the smallest ionization energy? Be (atomic# 4) Sr (atomic# 38) F (atomic# 9)…
Select the statement(s) that explain(s) the relationship between the arrangement of elements by size and first ionization energy. 1. The first set of paired electrons in a pp subshell experience a large amount of electron-electron repulsion, making the fourth electron in a pp subshell easy to remove. 2. The third unpaired electron in a pp subshell causes a lot of electron-electron repulsion among the orbitals, making the third electron in a pp subshell easy to remove. 3. A pp subshell with only one unpaired electron is extremely stable, making the fifth electron in a pp subshell easy to remove. 4. The two arrangements are the same because IE of elements increases from left to right and the radii of elements decreases from left to right. 5. A full ss subshell is able to shield a newly filled pp subshell from the nucleus, making the first electron in a pp subshell easy to remove.