Electrons in Atoms Dry Lab

Ionization energy decreases going down a group because _____. answer choices A.   Atoms are further away from the nucleus. B.   Effective nuclear charge increases C.   Effective nuclear charge decreases D.   The shielding effect stays the same. E.    There are more protons in the nucleus

Elements that have five electrons in the highest - energy p subleverl in their ground state are called ___________.

Atomic radius is defined as _______________ answer choices 1. One half the distance between two nuclei of two atoms of the same element bonded together 2. The atoms size 3. The distance from the nucleus to the outer edge of the electron cloud 4. The distance from the nucleus to the location of the highest occupied energy orbit

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2. Atomic radius _________ from left to right on the periodic table, and_________ top to bottom on the periodic table. a. decreases, increases b. increases, increases c. decrease, decreases d. increases, decreases   3. Which principle of electron distribution states that orbitals with lower energy must be filled up first? a. Hund's Ruleb. Pauli Exclusion Principlec. Coulomb's Lawd. Aufbau Principle   3. The following statements are from the Atomic Theory of Matter EXCEPT a. in chemical reactions, atoms are combined, separated, or rearranged atoms of a given element are identical in size, mass, and other propertiesb. atoms have overall neutral charge so there must be a source for both positive and negativechargesc. all statements are part of the Atomic Theory of Matterd. atoms cannot be subdivided, created, or destroyed

Pls help ASAP. Pls provide whether its true or false.

MY SCORE: b. Assessment /What I can show 7 7 Activity 8: "Gained or Lost" Directions: Indicate how many electrons must be gained or lost by each of the following atoms to achieve a stable electron configuration (Ex: 3 lost, 2 gained) 1. Sr 2. Sb 3. Xe 4. S 5. Se MY SCORE: D. Guide Questions Activity 11: "Question and Answer" Directions: Answer the following guide questions. ure?

NEED HELP TO SOLVE ATTACHED QUESTION. FROM STEPHEN STOKER CHEMISTRY BOOK CHAPTER-3.

All atoms are mostly ______ with the nucleus having a net charge of  _________.    A. empty space, negative   B. radioactive, polarized   C. empty space, zero   D. dense, positive   E. empty space, positive

First ionization energy ____down a group (i.e., top to bottom) on the periodic table.     a increases b decreases

Name: LIGHT, ELECTRON CONFIGURATION, AND PERIODIC TRENDS PRE-LABORATORY QUESTIONS 1. Explain the difference between a continuous spectrum and a discrete (line) spectrum. Include a sketch of each in the space below. Olucervetions dey 2. A traffic signal gives off green light, yellow light, and red light. Rank the colors in order, from highest to lowest energy. 3. In order to reduce "light pollution", many streetlights near observatories use sodium vapor lamps, which give off yellow light. a) Write the complete electron configuration for sodium. Incandscentght b b) How many valence electron(s) is/are found in sodium? Draw the electron dot formula for sodium. c) The wavelength of yellow light is about 550 nm. Using dimensional analysis, convert the wavelength to centimeters (cm). ucresce sht.blh the re ht the naked eye 4. Explain how you would clean the flame test wire in Part II. rough scope 5. List the safety precautions for Parts I and II. ved

3.The excited state of an electron ____________.   Question options:   possesses the same amount of potential energy as its ground stte   is unstable and very short-lived   ALL of these statements are accurate   is in the same orbital as its ground state   occurs when the electron enters the atomic nucleus

The atomic radius of main-group elements generally increases down a group because ________. a. the principal quantum number of the valence orbitals increases b. both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases c. effective nuclear charge increases down a group d. effective nuclear charge zigzags down a group e. effective nuclear charge decreases down a group

In metallic bond the atoms donate their electrons .This negative charge in turn _____________ the positively charged nucleus.

Give the "box notation" (also called the "dash notation") electron configuration of F- by filling electrons into the orbital spaces provided. Press Check when complete. Add either a single electron or a pair of electrons to an orbital by clicking and dragging the arrow symbol onto the dash. To remove electrons from an orbital, click on the orbital.

Objectives: a) Define Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. b) List and describe the four quantum numbers. c) Count valence electrons d) Write electron configurations

Remaining Time: 6 hours, 16 seconds. Question Completion Status: by side in a 0.50 g sample. How many miles in length is the line of chlorine atoms in the sample? 1 mi = 1609 m Attach File Browse Local Files QUESTION8 The table below is partially completed for subshells A and B, where subshell B is the next subshell higher in energy compared to subshell A. For example, if subshell A is 4s subshell, then subshell B would be the 3d subshell. Use these criteria and the information provided to complete the table. Subshell A Designation (1s, 3d, etc) Value of n Value of I Number of orbitals in subshell A Subshell B Designation (1s, 3d, etc) Value of n Value of I Number of orbitals in subshell A 4d 4 1 4 Attach File Browse Local Files QUESTION 9 An atom easily loses two electrons to form the ion R<*. The element, which is in Period 6, forms the oxides RO and RO2. Give the orbital diagram for the ground state valence shell of the element that immediately follows R in the periodic table.…

Elements that are most similar in their properties are found _____ A) in the same period. B) in the same group. C) have the same electron configurations. D) to occur randomly throughout the table. E) diametrically opposite each other on the periodic table.

_______  is the amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state.

rean d. Iron will not react in any nuclear reaction because of its stabilit Supernova has two key requirements: (1) the presence of an extreme Iron is the most stable element in temperature and (2) an abundant source of neutrons. Chapter Review ultiple Choice. Write the letter of the correct answer on the blank. 1. Which of the following is not true about iron? a. Iron is the twenty-sixth element in the periodic table. b. Iron can be found near the core of a massive star. c. Iron can be formed through stellar nucleosynthesis. d. Iron is very reactive in terms of nuclear reaction. 2. Which statement provides an explanation for your answer in No. a. Iron has 26 electrons and 26 protons. b. Iron cannot be found in the core because it has a low melting po c. Iron can only be formed in the surface of the sun. d. Iron will not react in any nuclear reaction because of its stabi 3. What is th ding block of all elements (excent hydrogen)?

Answer the dollowing pls