Periodic-Trends-Lab

Briefly explain the various scientists involved in the creation of the atomic model and what their view of the atom was Explain what the Quantum Mechanical model of the atom proposes Identify the number of protons/neutrons/electrons in a neutral element and in an ion Describe the different types of radioactive decay Calculate the average atomic mass of an element Define electronegativity, electron affinity, reactivity, atomic and ionic radius, ionization energy explain how each trend increases along a group and a column compare various elements to answer questions regarding C periodic trends Explain WHY a trend increases the way it does in a period or O group Interpret data of ionization energies Define the following: shielding effect, effective nuclear charge, the periodic law, cation, valence electrons, atomic mass, anion, energy levels(orbital), element, isotope, radioisotope

How do Group VIA elements form ions? A) They lose protons B) They gain two protons C) They lose two electrons D) They gain two electrons Which substance consists of anions and cations? A) CaF2, Calcium Fluoride B) Br2, Bromine C) Ag, Silver D) SiO2, Silicon Dioxide A newly discovered element is assigned to Group VIIA (Group 7A) in the periodic table. What charge will ions of this new element have? A) 1-    B) 2-    C) 1+    D) 2+ Reactions occur when atoms, ions or molecules collide. In a reaction between magnesium and bromine atoms, how many atoms of bromine will react per atom of magnesium? A) 1   B) 2   C) 3   D) 4 Which compound exists as a solid crystal lattice of cations and anions at room temperature? A) BrCl    B) CaCl2    C) SCl2    D) SiCl4

Using the terms atomic radius, and nuclear charge, explain why the elements on the right side of the periodic table typically have greater electronegativity value than those on the left side.

I do not understand

Please answer question 1 and 3 please let it be very short answers

The following Lewis diagram represents the valence electron configuration of a main-group element. This element is in what group in the periodic table? According to the octet rule, this element would be expected to form an ion with a charge of? If X is in period 5, the ion formed has the same electron configuration as the noble gas? What is the symbol for the ion?

1. How does ionization energy change as you move from left to right across a period? Explain r the representation of the periodic table below. Draw 2 arrows (next to and below) to represent increasing electronegativity. Ionization Energy your answer in terms of the number of protons in the nucleus 2. How does ionization energy change as you move from top to bottom in a group? Explain your answer in terms of energy levels. 3. On the representation of the periodic table below. Draw 2 arrows (next to and below) to represent increasing ionization energy.

How could we use the Bohr models to further elaborate the question about ionic bonds? Cite evidence from the image.

Back ground info:  Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron configuration ending with s2p6. One way an atom can satisfy the Octet Rule is by transferring valence…

Write the complete electron configuration for Cl- ion. What trend in electronegativity occurs as you go down a group on the periodic table? Explain why this occurs.  Write four quantum numbers to describe the highest energy electron in the Cl atom. The answer must include the four symbols and four correct numbers. Please answer all parts of question.

1. Arrange the following ions in order of increasing ionic radius: chloride ion, potassium ion, phosphide ion, calcium ion.

Pls help ASAP on all PLS I REQUEST

045 Worksheets Learning objectives Use position of element in periodic table to predict properties of elements Understand effective nuclear charge and its role in the size of an atom or ion and many other properties of elements Understand ionization energy and be able to predict trends Be able to predict higher/lower values of size, ionization energy, electron affinity, electronegativity and lattice energy Model 1 Repulsion Attraction The position of elements in the periodic table based on electron configuration creates a series of trends in behavior that are important r to understand as they affect many properties of elements. These properties are determined by the attraction of the outermost electrons to the protons in the nucleus and the electron-electron repulsion. Nucleus Z Outer electrons a. Trends Valence electrons b. You move down a column +3 This is known as Effective Nuclear Charge Compare sodium with aluminum. Which one would you predict to have a higher effective nuclear…

Write the full clectron configuration for P-. Bredback Start by determining the electron configuration of the neutral atom. full electron configuration: 1s2:°2p°3s°3p® Then, note whether electrons are gained or lost from the neutral atom electron configuration by looking at the ion charge. What is the atomic symbol for the noble gas that also has this clectron configuration? Lastly, add or remove electrons from the neutral configuration to form the ion configuration. atomic symbol: 18Ar40 Incerrect please explain than solvel

BALANCE the VALENCEComplete and fill out the table below. Find a non-metal element in the periodic table of elements which will completely cancel out the valence of the given element.

G The element in period 5 that has X akeCovalentActivity.do?locator assignment-take and lea X Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. The following Lewis diagram represents the valence electron configuration of a main-group element. •X. If this element is in period 5, its valence electron configuration is C Solved The following Lewis diagr X Retry Entire Group 9 more 8 CONS 144 G O Common Greek(upper) Greek(lower) Arrows Other XB Xu Aa (s) (1) (g) (aq) Undo Redo Clear Help L A + 0 Ox 0 0 + brt so backspace Previous Next> ENG P4D home Joci 12 ☆ 11:56 AM 11/28/2022 Rende 1 O bouq

Define the following terms and indicate how they behave within the periodic table of the elements, that is, how they increase or decrease depending on the groups and periods.Illustrate with graphs or figures. 1. Ionization energy2. Electron affinity (electronegativity),3. Atomic Radius4. Energy or ionization potential5. Electronegativity

Please provide only typed answer solution no handwritten solution needed

An unknown ionic compound is made of a monoanion and a monocation who both have the same electronic configuration as argon. Don't forget to indicate the physical state of each chemical species. A)what is the electronic configuration of argon? B)knowing the charge and electronic configuration of the ions, identify them. C)what are the electronic configuration of the parent elements? D)rank argon and the two parent elements by order of increasing radius. Explain your answer.

BALANCE the VALENCE Complete the table below. Find a nonmetal element in the periodic table of elements that will completely cancel out the valence of the given element

Answer question 7 or 8 please make your handwriting clear

1. Silicon has the electronic configuration 1s2 2s2 2p6 3s2 3p2.  Discuss how you can determine that 1s2 2s2 2p6 3s2 3p2 is the electronic configuration for silicon. 2. What is a reason potassium tends to lose one electron to form a +1 ion K+1?  What is the reason chlorine tends to add one electron to form the -1 ion Cl-1 ?  Hint:  They are the same reason. 3. In the abbreviated electronic figure for phosphorus [Ar] 3s2 3p3 how do you know what are the core electrons?   4. A student got a problem wrong.  They were asked,  “How many grams of MgCl2 (molar mass = 95.21 g/mol) are needed to make 3.16 L of a 0.500 M MgCl2 solution?”  The correct answer is 150. but the student got 1.58.  What mistake did the student make? 5. To solve the following problem what is the reason you must subtract the vapor pressure of water, 24 torr, from the total pressure, 747 torr in order to solve the problem? “A 500.0-mL sample of H2 gas is collected over water at 298 K and 747 torr.  What volume would the…

What is the difference for a bicentric and a bielectronic covalent bond?

3. Write a chemical equation corresponding to the second ionization energy of calcium.

The following Lewis diagram represents the valence electron configuration of a main-group element. X: This element is in group 2A According to the octet rule, this element would be expected to form a(n) cation with a charge of +2 If X is in period 5 , the ion formed has the same electron configuration as the noble Kr gas The symbol for the ion is

You have just discovered a new element, "Zoomfatigueium" (Zo). It's a non-metal that has similar properties to those elements in Group 14 of the periodic table. The following questions are about species containing this element. 1) If Zo can be found in Group 14, then how many valence electrons does it have? 2) Zo forms a polyatomic ion with the formula Zo03 called the "youremuted ion." You are not sure of its charge until you discover that it forms the ionic compound MgZoO3. What must be the charge of the youremuted ion? 3) Draw a plausible Lewis structure for the yourmuted ion, using the answer to Question 2 to guide how many valence electrons must be represented in the structure. 4) Based on your answer to Question 3, answer the following questions about the youremuted ion: a. Molecular geometry of Zo b. Hybridization of Zo 0- Zo -0 bond angles C. 5) The Zo - O single bond has a length of 143 pm while the Zo -0 double bond has a length of 123 pm. In the youremuted ion, the Zo - O…

Identify and encircle the element that has the greater ionization energy. 1. indium and cobalt2. tellurium and aluminum 3. germanium and oxygen

1.)

The following Lewis diagram represents the valence electron configuration of a main-group element. X• This element is in group According to the octet rule, this element would be expected to form a(n) with a charge of If X is in period 3 , the ion formed has the same electron configuration as the noble gas CO The symbol for the ion is

Give detailed Solution with explanation needed..don't give Handwritten answer

Question: Consider the periodic table and its arrangement of elements. The elements are organized based on their atomic number and similar chemical properties. Using your understanding of periodic properties in chemistry, answer the following tough logical reasoning question: If Element A has a higher atomic number than Element B, and Element B is located in Group 2 of the periodic table, what can you infer about the following properties of these elements? a) Atomic radiusb) Ionization energyc) Electronegativity Explain your reasoning for each property and provide your answers.

ome OWLV2 | Online teaching and learning resource from Cengage Learning [References] Use the References to access important values if needed for this question. The following Lewis diagram represents the valence electron configuration of a main-group element. The element in period 3 that has this valence electron congfiguration is 1A 8A H 2A 3A 4A 5A 6A 7A He Li Be B CNO F Ne Na Mg 3B 4B 5B 6B 7B 1B 2B Al Si P S CI Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg TI Pb Bi Po At Rn Fr Ra Ac Rf Ha Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa UNp Pu Am Cm Bk Cf Es Fm Md No Lr

Please answer question 2