can someone help me to answer those questions
Homework Answers
17 a. The graph represents the 1st ionization energy of atoms. Ionization energy is the amount of energy required to remove an electron from the outermost shell of an isolated gaseous atom.
17 b. The four lines represents the increasing trend of ionization energy of the columns or groups of the periodic table.
18 . The ionization energy generally increases on moving left to right across a period .
19. The ionization energy generally decreases on moving top to botttom down the group.
20. No the trends are not perfect. The bips or discrepencies in the trends are due to
- Nuclear charge: the greater the magnitude of nuclear charge the more tightly the electrons are held by the nucleus and hence more will be ionization energy.
- Number of electron shells: the greater the size of the atom, the less tightly the electrons are held by the nucleus and ionization energy will be less.
- Effective nuclear charge (Zeff): the greater the magnitude of electron shielding and penetration the less tightly the electrons are held by the nucleus, the lower the Zeff of the electron, and hence less will be the ionization energy.[4]
- Type of orbital ionized: the atom having a more stable electronic configuration has less tendency to lose electrons and consequently has high ionization energy.
- Occupancy of the orbital matters: if the orbital is half or completely filled then it is harder to remove electrons
No they do not always occur in the same place.
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can someone help me to answer those questions
N Ctrl Extension Questions Model 3 - Ionization...
can someone help me to answer those questions 8. Explain the trend as you move across...
can someone help me to answer those questions
8. Explain the trend as you move across a row of the periodic table for each of the following some properties using your understanding of effective nuclear charge. Atomic radius b. Ionization energy 6. Electronegativity STOP Model 2 - The Alkali Metals Pare Atomic Number Core Charge Atomic Radius 1st lonization Energy Electro- negativity Lithium 0.91 Sodium 152 pm 186 pm 227 pm 520 kJ/mole 496 kJ/mole 419 kJ/mole 0.87 0.73 Potassium...
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...
- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions:...
- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions: Please answer each fill in the blank with the best answer. 1. The energy required to remove an electron from a gaseous atom is called the T ilas_energy. 2. When an electron is removed the atom gets a 3. The energy required to remove a second electrons is called the charge. energy. 4. It always requirest i -- to remove a second electron. 5....
Can someone explain the graph to me I dont know how to read it to answer the questions
can someone explain the graph to me I dont know how to
read it to answer the questions
Atomic radius Nbonding The radius of an atom describes the distance between the nucleus and the outermost electron. This distance is very small so it is often reported in picometers (101 m) or angstroms (10-10 m). One way of measuring the atomic radius is to observe the distanc between bonding atoms. The distance between the nuclei of the bonding atoms is equal...
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....
3. Electronegativity (the ability of an atom to pull electrons toward itself in a chemical bond) and Ionization Ene...
3. Electronegativity (the ability of an atom to pull electrons toward itself in a chemical bond) and Ionization Energy (the amount of energy required to remove an electron from an atom) have the same trend on the periodic table. The largest electronegativities and ionization energies are found in the region of the periodic table. Report the letter (A, B, C, etc) of your answer in the space beside the question number. A. upper left B. upper right C. lower left...
Font Paragraph F Styles Data Sheet Table 1: Periodic Trends Periodicity Observation What are the Group...
Font Paragraph F Styles Data Sheet Table 1: Periodic Trends Periodicity Observation What are the Group 1 elements called? Within a group, what happens to the atomic radius as you go down the column? Within a period, what happens to the atomic radius as the atomic number increases? What is the general trend of electronegativity as you go left to right across the periodic table? What is the general trend of electronegativity as you go down the periodic table? What...
I need help with all these questions. Please and thank you 1. An element has the...
I need help with all these questions. Please and thank you
1. An element has the following electronic configuration: [Kr]4d5552 (a) What period does it belong to? (b) What is its group number? (Use group numbers from 1 to 18) (c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?) (d) How many unpaired electrons are there in an atom of this element? (a) What element has this electronic configuration? 1s 2s 2p 3s2 (b) What...
Can someone help me answer questions B and C from the last page of the lab....
Can
someone help me answer questions B and C from the last page of the
lab. Please
T-Mobile 10:30 p. m. a learn.vccs.edu KINETIC AND POTENTIAL ENERGY Please at the end of the lab experiment clean your table and wait for the instructor to check you out! All the group partners must be present. Thank you. Lab's goal In this experiment we will determine the Kinetic (K) and Potential Energy (U) of a cart moving down an incline. We will...
Problem Set 4 Atomic Structure and the Periodic Table Name: Date: Lab Section: General Instructions Complete the f...
Problem Set 4 Atomic Structure and the Periodic Table Name: Date: Lab Section: General Instructions Complete the following problems. Attach another sheet to give yourself space for problems 8,9,10 as needed. Assignment is due at the end of the lab period unless stated otherwise by instructor. 1.) Energy Levels and Sublevels for the Polyelectronic Atom (a) How many sublevels exist in the energy level (n = 5)? (b) How many orbitals exist in any f-sublevel? (c) What is the maximum...
can someone help me to answer those questions
8. Explain the trend as you move across a row of the periodic table for each of the following some properties using your understanding of effective nuclear charge. Atomic radius b. Ionization energy 6. Electronegativity STOP Model 2 - The Alkali Metals Pare Atomic Number Core Charge Atomic Radius 1st lonization Energy Electro- negativity Lithium 0.91 Sodium 152 pm 186 pm 227 pm 520 kJ/mole 496 kJ/mole 419 kJ/mole 0.87 0.73 Potassium...
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...
- Class period! Unit 4: Periodic Trends "lonization Energy Trend" - Wksh # 4 2 Directions: Please answer each fill in the blank with the best answer. 1. The energy required to remove an electron from a gaseous atom is called the T ilas_energy. 2. When an electron is removed the atom gets a 3. The energy required to remove a second electrons is called the charge. energy. 4. It always requirest i -- to remove a second electron. 5....
can someone explain the graph to me I dont know how to
read it to answer the questions
Atomic radius Nbonding The radius of an atom describes the distance between the nucleus and the outermost electron. This distance is very small so it is often reported in picometers (101 m) or angstroms (10-10 m). One way of measuring the atomic radius is to observe the distanc between bonding atoms. The distance between the nuclei of the bonding atoms is equal...
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....
3. Electronegativity (the ability of an atom to pull electrons toward itself in a chemical bond) and Ionization Energy (the amount of energy required to remove an electron from an atom) have the same trend on the periodic table. The largest electronegativities and ionization energies are found in the region of the periodic table. Report the letter (A, B, C, etc) of your answer in the space beside the question number. A. upper left B. upper right C. lower left...
Font Paragraph F Styles Data Sheet Table 1: Periodic Trends Periodicity Observation What are the Group 1 elements called? Within a group, what happens to the atomic radius as you go down the column? Within a period, what happens to the atomic radius as the atomic number increases? What is the general trend of electronegativity as you go left to right across the periodic table? What is the general trend of electronegativity as you go down the periodic table? What...
I need help with all these questions. Please and thank you
1. An element has the following electronic configuration: [Kr]4d5552 (a) What period does it belong to? (b) What is its group number? (Use group numbers from 1 to 18) (c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?) (d) How many unpaired electrons are there in an atom of this element? (a) What element has this electronic configuration? 1s 2s 2p 3s2 (b) What...
Can
someone help me answer questions B and C from the last page of the
lab. Please
T-Mobile 10:30 p. m. a learn.vccs.edu KINETIC AND POTENTIAL ENERGY Please at the end of the lab experiment clean your table and wait for the instructor to check you out! All the group partners must be present. Thank you. Lab's goal In this experiment we will determine the Kinetic (K) and Potential Energy (U) of a cart moving down an incline. We will...
Problem Set 4 Atomic Structure and the Periodic Table Name: Date: Lab Section: General Instructions Complete the following problems. Attach another sheet to give yourself space for problems 8,9,10 as needed. Assignment is due at the end of the lab period unless stated otherwise by instructor. 1.) Energy Levels and Sublevels for the Polyelectronic Atom (a) How many sublevels exist in the energy level (n = 5)? (b) How many orbitals exist in any f-sublevel? (c) What is the maximum...
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