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1. Compare the first ionization energy of Ca to that of Zn. Justify these values using...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
Explain the definition of ionization energy, the observed group and period trends for this property, and...
Explain the definition of ionization energy, the observed group and period trends for this property, and (using effective nuclear charge) why the observed trends happen the way they happen. For each of the following molecules, draw a Lewis structure (all resonance structures if necessary), indicate the molecular geometry, and indicate the bond angles based on VSEPR theory: Identify the hybrid orbitals used for each of the following geometries, according to Valance Bond Theory: (a) tetrahedral _____ (b) bent (as in...
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or...
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or ion in the gaseous state. The ionization energy is always positive because it takes energy to remove and electron. 1) Using the figure on the left, which elements have the highest first ionization energies? 2) Does this make sense as to why they have high Ionization energy? ell tentation energi 3) Which elements have the lowest first ionization energies? 4 Does this make sense...
Ionization energy (Ei) is the amount of energy required to remove an electron from a neutral...
Ionization energy (Ei) is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. Electrons are attracted to the positively charged nucleus; therefore removing an electron requires energy. The process is endothermic, and so ionization energies have a positive value. The first ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom. The reaction is represented for the generalized atom X as X→X++e− The amount...
7. Answer each of the following using only the periodic trends. a. Circle the atom with...
7. Answer each of the following using only the periodic trends. a. Circle the atom with the larger atomic radius, Na or Si. b. Circle the atom with the larger lonization Energy, 0 or S. c. Circle the atom with the more favorable Electron Affinity, I or Br. d. Circle the atom with the largest Effect Nuclear charge, Be or N. e. Circle the atom with the largest Electronegativity, S or P. 8. Answer each of the following using only...
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first?...
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first? Second ionization energy is always 4 times greater than the first. After removal of the second electron, rubidium has a configuration of noble gas. The second electron is removed from 4p, which is much closer to the nucleus than 58, Rb has a configuration of noble gas, which is stable. Submit What experiments could be done to provide some evidence that the correct formulation...
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5)...
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5) Which element has the highest electron affinity? A) Ge В) 0 С) в D) Ca E)K 6) of the 3 elements fluorine, bromine, and calcium, has the highest ionization energy and _has the lowest ionization energy. (Note that we are considering the first ionization energy). A) bromine; calcium B) calcium; fluorine C) fluorine; bromine D) fluorine; calcium E) none of these 7) Based upon...
please help with question 1 and 2 THANK YOU IN ADVANCE 1. Complete the table below...
please help with question 1 and 2 THANK YOU IN ADVANCE
1. Complete the table below with information about properties of elements on the periodic table. (2.5 pts) Property Definition Trend from Left to Right across a period Trend from top to bottom down a group Atomic Radius Ionic Radius I First Ionization Energy Electron Affinity Number of Valence Electrons 2. For the elements listed below, predict what the ionic charge will be and write the electron configuration for the...
1. Identify the atomic number, first ionization energy, electronegativity, and the atomic radius of barium, chlorine,...
1. Identify the atomic number, first ionization energy, electronegativity, and the atomic radius of barium, chlorine, and nitrogen. What can you observe about the trends of these properties? 2. Copper is typically used in electrical work. What type of material is it? What properties allow it to perform well? Why is sulfur not used in electrical wires? 3. Explain the connection between allotropes and the types of element.
Give the name of the element fitting each of the following descriptions. a. The element whose...
Give the name of the element fitting each of the following descriptions. a. The element whose +3 cation has the same configuration as krypton. b. The element whose -2 anion has the same configuration as xenon. c. The element from the first 10 elements that would be most similar in properties to franicum. d. The Period 2 element having 4 valence electrons. e. The Period 4 element having a half filled p subshell in the valence shell. f. The Period...
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
Explain the definition of ionization energy, the observed group and period trends for this property, and (using effective nuclear charge) why the observed trends happen the way they happen. For each of the following molecules, draw a Lewis structure (all resonance structures if necessary), indicate the molecular geometry, and indicate the bond angles based on VSEPR theory: Identify the hybrid orbitals used for each of the following geometries, according to Valance Bond Theory: (a) tetrahedral _____ (b) bent (as in...
Ionization energy Ionization Energy is the energy required to remove an electron from an atom or ion in the gaseous state. The ionization energy is always positive because it takes energy to remove and electron. 1) Using the figure on the left, which elements have the highest first ionization energies? 2) Does this make sense as to why they have high Ionization energy? ell tentation energi 3) Which elements have the lowest first ionization energies? 4 Does this make sense...
7. Answer each of the following using only the periodic trends. a. Circle the atom with the larger atomic radius, Na or Si. b. Circle the atom with the larger lonization Energy, 0 or S. c. Circle the atom with the more favorable Electron Affinity, I or Br. d. Circle the atom with the largest Effect Nuclear charge, Be or N. e. Circle the atom with the largest Electronegativity, S or P. 8. Answer each of the following using only...
Rb : [kr] Rb++[Ar]4323d104p) b Why is the second ionization energy much greater than the first? Second ionization energy is always 4 times greater than the first. After removal of the second electron, rubidium has a configuration of noble gas. The second electron is removed from 4p, which is much closer to the nucleus than 58, Rb has a configuration of noble gas, which is stable. Submit What experiments could be done to provide some evidence that the correct formulation...
4) Which element has the highest electronegativity? A) Ge B) O C) B D) Ca 5) Which element has the highest electron affinity? A) Ge В) 0 С) в D) Ca E)K 6) of the 3 elements fluorine, bromine, and calcium, has the highest ionization energy and _has the lowest ionization energy. (Note that we are considering the first ionization energy). A) bromine; calcium B) calcium; fluorine C) fluorine; bromine D) fluorine; calcium E) none of these 7) Based upon...
please help with question 1 and 2 THANK YOU IN ADVANCE
1. Complete the table below with information about properties of elements on the periodic table. (2.5 pts) Property Definition Trend from Left to Right across a period Trend from top to bottom down a group Atomic Radius Ionic Radius I First Ionization Energy Electron Affinity Number of Valence Electrons 2. For the elements listed below, predict what the ionic charge will be and write the electron configuration for the...
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