Connect Assignment: Chapter 7 Electron Structure of the Atom

using the electromagnetic spectrum (shown) match each frequency of light to the correct region

- 1 x10^17 s^-1: x-ray - 1 x10^13 s^-1: infrared - 1 x10^11 s^-1: microwave - 1 x10^7 s^-1: radio frequency - 1 x10^15 s^-1: ultraviolet

match all the elements or ions that are isoelectronic

- Br^- : Kr - Ca^2+ : Ar - Na^+ : F^- - He : Li^+

match each symbol to the correct value and/or units

- E photon: units of J or J/photon - h: 6.626 x 10^-34 Js - c: 3.00 x 10^8 m/s - ʎ: units of m - v: units of s^-1, 1/s, or hertz (Hz)

match each main-group element to find the correct number of valence electrons present

- P: 5 - F : 7 - Si: 4 - H: 1 - Ar: 8

match each electron configuration to the element it represents. the orbital diagram (shown) may be used

- Zn (Z = 30): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 - P (Z = 15): ): 1s^2 2s^2 2p^6 3s^2 3p^3 - Ca (Z = 20): ): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 - Ga (Z = 31): ): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^1

match the electron configuration to the number of electrons needed to be lost or gained to acquire a stable noble gas electron configuration

- [Ne] 3s^2 3p^5: add 1 more electron to acquire a stable noble gas electron configuration -[Ne] 3s^2: loses 2 electrons to acquire a stable noble gas electron configuration -[Ar] 4s^1: lose 1 electron to acquire a stable noble gas electron configuration -[He]: has a stable noble gas electron configuration - [Ne} 3s^2 3p^4: gain 2 electrons to acquire a stable noble gas electron configuration

select all the statements that correctly describe trends in atomic radii for ions

- a cation is smaller than its neutral atom because the protons draw the remaining electrons closer to the nucleus - an anion is larger than its neutral atom because the protons cannot hold the increased number of electrons as close to the nucleus

select all the statements that correctly describe photons and/or photon energy

- a photon a packet of light energy - light of only one wavelength consists of photons of identical energy

select all the options that correctly relate the line spectrum of hydrogen to the Bohr model of the atom (figure shown)

- a transition to the n=2 orbit from a higher-energy orbit in some cases produces an emission of visible light - the energy between two orbits [△E] is equal to the energy of the photon emitted or absorbed Ephoton in an electron transition

select all the statements that correctly describe periodic trends in ionization energies (IE)

- across a row, valence electrons are more attracted to the nucleus because of the increased number of protons (IE increase) - going down a group, valence electrons are farther from the nucleus and are easier to remove (IE decreases) - going down a group, valence electrons are increasingly shielded from the nucleus by core electrons and are easier to remove (IE decreases)

match each group of elements to the correct chemical reactivity trend observed based on valence electrons

- alkali metals (group IA): react chemically to lose 1 valence electron to acquire a stable noble gas electron configuration - alkaline earth metals (group IIA): react chemically to lose 2 valence electrons to acquire a stable noble gas electron configuration - halogens (group VIIA): react chemically to gain 1 valence electron to acquire a stable noble gas electron configuration - noble gases (group VIIIA): have filled valence s and p sub levels and are highly stable and typically do not react chemically

match each type of metal with the correct statement

- alkali metals: metals that are commonly found as 1+ ions in nature - alkaline earth metals: metals that are commonly found as 2+ ions in nature

select all the options that correctly describe the configuration of electrons in an atom

- an atom in its ground state contains electrons that are in the lowest-energy configuration possible -electrons are filled into orbitals starting with the lowest-energy orbitals and "build up" to higher-energy orbitals

select all the options that correctly describe electron configuration

- an electron configuration describes the arrangement of electrons in an atom - an electron configuration shows the distribution of electrons among sublevels

select all the statements that correctly describe the electron configuration of ions

- anions have more electrons that protons, and cations have fewer electrons than protons - for each negative charge on an ion of a given element, an electron must be added to the configuration of the atom

match each term concerning spectra to the definition

- continuous spectrum: a sequence of colors that contains all the wavelengths of light in the visible region - white light: all the wavelengths of the visible spectrum at equal intensity - line spectrum: a set of distinct wavelengths of light that is unique for each element

select all the options that correctly describe electromagnetic radiation

- electromagnetic radiation travels through space as oscillating waves - energy in the form of light is called electromagnetic radiation - electromagnetic radiation consists of oscillating electric and magnetic fields

select all the options that correctly describe frequency

- frequency is described in units of s^-1, 1/s, or hertz (Hz) - frequency is a measure of the number of wave cycles that move through a point in space in 1 second - frequency is symbolized by the Greek letter nu, v

match each term with the correct description for arranging electrons in an atom

- ground state: the lowest-energy state of the atom - aufbau principle: electrons fill orbitals starting with the lowest-energy orbitals - pauli exclusion principle: a maximum of two electrons can occupy each orbital, and they must have opposite spins - Hund's rules: electrons are distributed into orbitals of identical energy in such a way as to give the maximum number of unpaired electrons

which of the following trends concerning ionization energies and the main-group elements are correct? select all that apply

- ionization energies generally increase from left to right across the periodic table - the highest ionization energies are observed for the elements in the upper right corner of the periodic table

select all the correct statements concerning valence electrons of elements

- main-group elements in the same group of the periodic table have the same number of valence electrons - the valence electrons of an atom all reside in the same principal energy level, n - for any main-group element, the number of valence electrons is equal to the number of electrons in the highest-energy s and p sublevels

match each principal energy level with all the orbitals found on that level

- n=1 : s only - n=2 : s and p only - n=3 : s, p, and d only - n=4 : s, p, d, and f only

match each sublevel to the correct description

- s: a single orbital that is in the shape of a sphere - p: three orbitals that are each in the shape of a dumbbell - d: five orbitals, in which four of them have four lobes and one of them has two lobes - f: seven orbitals, found only on the fourth principal energy level and above

select all the options that correctly relate electron transitions to change of energy in the Bohr model of the hydrogen atom

- the difference in energies between two different orbits is represented by △E = Efinal - Einitial - an electron is an orbit close to the nucleus can absorb energy and move to a higher-energy orbit that is farther from the nucleus

which of the following is correct concerning the principal energy level (n)? select all that apply

- the first principal energy level (n = 1) consists of only one orbital - higher principal energy levels consists of more orbitals than lower principal energy levels

select all the options that correctly describe the principle energy level (n)

- the larger the numerical value of the principal energy level (n), the larger the orbital size - the principal energy level (n) is represented with a positive integer

select all the statements that correctly describe the role of valence electrons in chemical reactivity

- the number of valence electrons lost or gained to adopt a noble gas configuration governs what ions are formed by main-group elements - valence electrons are the electrons that participate in chemical reactions because they are the farthest from the nucleus - filled valence s and p sublevels give exceptional stability to any atom or ion

which of the following options explains why the second ionization energy for Li is 7298 kJ/mol, whereas the second ionization energy for Be is 1757 kJ/mol? select all that apply

- the second electron removed from Be is a valence electron, which requires much less energy than removal of core electrons - the second electron removed from Li is a core electron, which requires much more energy than removal of valence electrons

select all the options that correctly compare waves A and B (shown)

- wave A has a higher frequency than wave B - wave A has a higher energy than wave B

select all the options that correctly describe the speed of light (c)

- x-rays, ultraviolet light, and microwaves all travel at the same speed when in a vacuum - the speed of light, c, is equal to 3.0 x 10^8 m/s

match each equation to the process involved for the ionization energy that is represented (M=metal)

-M(g) -> M^+(g) + e^- : first ionization energy -M^+(g) -> M^2+(g) + e^- : second ionization energy -M^2+(g) -> M^3+(g) + e^- : third ionization energy

use the orbital diagrams (shown) to list the following sublevels in order of decreasing energy. the highest-energy sublevel belongs at the top of the list

1. 4p 2. 3d 3. 4s 4. 3p 5. 3s

list the following elements in order of increasing ionization energy. the element with the smallest ionization energy belongs at the top of the list

1. K 2. Br 3. Cl 4. F 5. He

list the following elements in order to increasing ionization energy. the element with the smallest ionization energy belongs at the top of the list

1. K 2. Ge 3. As 4. Br 5. Kr

list the following atoms or ions in order of increasing atomic radii. the atom or ion with the smallest atomic radius belongs at the top of the list

1. Li^+ 2. Li 3. Cl^- 4. P^3-

list the following electron configurations in order of increasing size concerning the neutral atoms they represent. the smallest neutral atom represented belongs at the top of the list

1. [He] 2s^2 2. [Ne] 3s^2 3. [Ar] 4s^2 4. [Kr] 5s^2 5. [Xe] 6s^2

list the following types of electromagnetic radiation (spectrum shown in figure) in order of increasing wavelength. the light with the shortest wavelength belongs at the top of the list

1. gamma ray 2. ultraviolet 3. visible 4. microwave 5. radio frequency

list the steps in chronological order concerning how to write an abbreviated electron configuration for an element.

1. locate the position of the element on the periodic table 2. find the closest noble gas in the period above the element 3. write the symbol of the noble gas in brackets 4. add the additional electron configuration needed to reach the element on the periodic table

use the periodic table (shown) to write the electron configuration for Sn (Z = 50)

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^2

the valence electrons for S (Z = 16) are represented by which of the following options?

3s^2 3p^4

what is the total number of electrons that can occupy the 5p sublevel?

6

calculate the wavelength of light, in. units of nanometers, with a frequency of 4.36 x 10^15 Hz

68.8 nm

the ionization process for which ionization energy is measured is represented by which of the following equations? (M = any metal)

M(g) -> M^+(g) + e^-

which of the following options correctly describes the core and valence electrons for Ge ([Ar] 4s^2 3d^10 4p^2)?

[Ar] 3d^10 includes the core electrons and 4s^2 4p^2 represents the valence electrons

which of the following represents the electron configuration of S^2- (Z = 16)?

[Ne] 3s^2 3p^6

which of the following options correctly describes orbitals?

an orbital is a region of space in which an electron is likely to be found

what type of electromagnetic radiation is light with a wavelength of 10 meters? use the electromagnetic spectrum shown

radio frequency

which of the following options correctly explains why the orbital diagram (shown) of the ground-state configuration for nitrogen (Z=7) is incorrect?

the Aufbau principle is violated, the lowest-energy orbitals are not filled before the higher-energy orbitals

which of the following statements correctly describes how atomic radii are measured for most atoms?

the distance between the centers of two identical bonded atoms is measured. the atomic radius is one-half this distance

which of the following options describes the fundamental idea of the Bohr model?

the energies of electrons in an atom are quantized, they can only have certain values