Chem Exam #2
name three observed properties associated with how atoms interact with electromagnetic radiation can NOT be explained by waves:
1. The emission of light from hot objects(blackbody radiation) 2. the emission of electrons from metal surfaces on which light is shone(the photoelectric effect) 3.emission of light from electronically excited gas atoms(emission spectra)
Niels Bohr adopted Planck's assumption and explained these phenomena in this way(name three key ways):
1.Only orbits of certain radii, corresponding to specific energies, are permitted for the electron in a hydrogen atom. An electron in a permitted orbit is in an "allowed" energy state. An electron in an allowed energy state does not radiate energy, and, therefore, does not spiral into the nucleus. Energy is emitted or absorbed by the electron only as the electron changes from one energy state to another. This energy is emitter or absorbed as a photon that has energy E = hν. (energy of the photon(E)+Planck's constant , 6.626x10^-34 JS (h) x frequency of the photon(v)
give the electron configuration of: p3-
1s22s22p63s23p6
nm(nanometer)=
1x10^-9
Which atom has the electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d7?
27 Co
how many valence electrons does carbon have?
4, because its in group 4!
define ionic bond
A compound that contains ions and is held together by ionic bonds is called an ionic compound.
give the nobles gas configuration of: 37 Rb
(Kr) 5s1
The Photoelectric Effect
-Einstein used quanta to explain the photoelectric effect -Each metal has a different energy which it ejects electrons. At lower energy, electrons are not emitted. -He concluded that energy is proportional to frequency *E = hν*
how many valence electrons in K or potassium?
1 because its in group one
remember + as a charge or ion you subrtract and - as a charge or ion means you add, please dont trip up on this. the opposite is what you do.
electron configuration ex. Na+ = 1s22s22p6 (you took away an electron)
what are the main group elements:
groups 1, 2, and 13-18
what groups are the transition metals:
groups 3-12
what is the magnetic quantum number
ml
how can you determine the size of the radius of an element
moving to the right = decreases and moving down = increases
what is the spin quantum number
ms
what is the principal quantum number
n
what is the principal quantum shell letter
n
N:The principal quantum number, ___, describes the energy level on which the orbital resides. The values of ___ are integers ≥ 1.
n principal quantum number
s=
solid
what designates the number of electrons in a particular subshell?
the subscript!
Define amplitude
Corresponds to the magnitude of the waves displacement
_______ developed a mathematical treatment into which both the wave and particle nature of matter could be incorporated. This is known as__________.
Erwin Schrödinger developed a mathematical treatment into which both the wave and particle nature of matter could be incorporated. This is known as quantum mechanics.
First ionization energies_______down a group and ________across a period
First ionization energies: Decrease down a group Increase across a period
Define Frequency
Frequency is the number of wave cycles that pass a specific point in a space in a specified amount of time unit for frequency, expressed as cycles per second [s−1] is the hertz (Hz)
what has the shortest wavelength
Gamma Rays
how do you find valence electrons?
In a neutral atom valence electrons are equal to the group number
quantum numbers of electrons in atoms
LOOK AT PIC STUDY PIC
Unlike n ,l and ml the electron spin quantum number ms does not depend on another quantum number. It designates the direction of the electron spin and may have a spin of +1/2, represented by↑, or -1/2, represented by ↓. This means that when ms is positive the electron has an upward spin, which can be referred to as "spin up." When it is negative, the electron has a downward spin, so it is "spin down.
Spin quantum number MS
The first _____ quantum numbers define the orbital and the ______ quantum number describes the intrinsic electron property called ____.
The first three quantum numbers define the orbital and the fourth quantum number describes the intrinsic electron property called spin.
what side are the reactants on?
The left, reactants=product
The notation 2p^4 (read "two-p-four") indicates four electrons in a p subshell (l = ___) with a principal quantum number (n) of ___.
The notation 2p4 (read "two-p-four") indicates four electrons in a p subshell (l = 1) with a principal quantum number (n) of 2.
The solution of Schrödinger's wave equation for hydrogen yields_________for the electron.
The solution of Schrödinger's wave equation for hydrogen yields wave functions for the electron.
The square of the wave function gives the__________, or probability of where an electron is likely to be at any given time.
The square of the wave function gives the electron density, or probability of where an electron is likely to be at any given time.
To determine the electron configuration for an atom we add a number of electrons equal to its atomic number: what is this procedure called?
This procedure is called the Aufbau principle!
Thus, the attraction to the nucleus is ______ and the energy associated with the orbital is ______ (less stabilized).
Thus, the attraction to the nucleus is weaker and the energy associated with the orbital is higher (less stabilized).
true or false: Hydrogen is a non metal?
True, Hydrogen has a special property and is a non metal
quantum number
Value of L: 0=s 1=p 2=d 3=f (n=1 can have only one l number and it is labelled l = 0 n=2 can ha ve two l numbers and labeled as l=0 and l= 1 n= 3 can have 3 l numbers and labeled as l= 0, l=1 and l=2)
Give the formula for the first ionization energy:
X(g) ⟶ X^+(g) + e^− IE1
_____ is when two or more substances react to form one single product
a combustion reaction is when two or more substances react to form one product ex. A+B=C
what is a molecular(aka covalent) compound
a compound that contains a non metal
what is an ionic compound
a compound that has a metal in it
give the nobles gas configuration of: 23 V
(Ar) 3d3 4s2
give the nobles gas configuration of: 13 Al
(Ne) 3s2 3p1
give the nobles gas configuration of: 17 Cl
(Ne) 3s2 3p5
all waves, including forms of electromagnetic radiation, are characterized by: (name three)
-Wavelength(λ) -Frequency(ν) -Amplitude
Name two important ideas in the bohr model
1. Electrons exist only in certain discrete energy levels, which are described by quantum numbers 2. Energy is involved in the transition of an electron from one level to another
list the first 7 electrron order filling the orbitals
1s, 2s, 2p, 3s, 3p, 4s, 3d
write the order of electron filling to the orbitals: hint 1s, 2s....
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s
give the electron configuration of: al 2+
1s22s22p63s1
Which atom has the electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d 2?
40 Zr
Write out Planck's constant
6.626x10^-34 Js (Joule seconds)
_______ is a positively charged ion that forms when one or more electrons are removed from the atom
A cation (positively charged ion) forms when one or more electrons are removed from an atom.
________is a negatively charged ion that forms when one or more electrons are added to a parent atom
An anion (negatively charged ion) forms when one or more electrons are added to a parent atom.
An ________ in an atom is completely described by four quantum numbers: __ - Principal quantum number __- Angular quantum number __ - Magnetic quantum number __ - Spin quantum number
An electron in an atom is completely described by four quantum numbers: n - Principal quantum number l - Angular quantum number ml - Magnetic quantum number ms - Spin quantum number
An orbital is described by a set of_______quantum numbers.
An orbital is described by a set of three quantum numbers.
name three examples of metalloids
Anything on the first four steps, B, Si, As, Sb, Te, including Ge etc
determine the relationship between frequency and wavelength
As wavelength increases, frequency increases (and vice versa)
Based on their positions in the periodic table, predict which has the smallest atomic radius: Mg, Sr, Si, Cl, I.
Cl
what do combustion reactions usually produce?
Combustion reactions usually produce rapid reactions that produce a flame and most often involve air as a reactant
_______ Mendeleev in Russia (1869) and _______Meyer in Germany (1870) independently recognized that there was a periodic relationship among the properties of the elements known at that time.
Dimitri Mendeleev in Russia (1869) and Lothar Meyer in Germany (1870) independently recognized that there was a periodic relationship among the properties of the elements known at that time.
write out the formula: E = hν
E-Energy of photon = h-Planck's constant (6.626 x 10^-34 J∙s ) x ν-frequency of the photon
the element name is the top left, the number of electrons is the top right, and the subshell is the group(the middle)
Ex. Hydrogen with the h in the top left, the electrons in the top right(1) and the group or subshell 1s in the middle
give the electron configuration of: fe 2+
Fe2+: 1s22s22p63s23p63d6
Beginning with hydrogen, and continuing across the periods of the periodic table, we add one electron to the subshell of lowest available energy. what is the electron configuration of fluorine? hint: we add one electron every time we move
Fluorine= 2p^5
write the electron configuration of H and the arrows
H - 1s^1 - arrow up - so plus 1/2
name three examples of nonmetals
H, He, Br, Kr, Hydrogen and the top far right of the periodic table
write the electron configuration of He and the arrows
He - 1s^2 - arrow up, arrow down - so negative1/2
Give the name of who created this rule: The lowest energy configuration for an atom with electrons within a set of degenerate orbitals is that having a maximum number of unpaired electrons
Hund's rule
I: This quantum number defines the shape of the orbital. Allowed values of l are integers ranging from 0 to n − 1. Letter designate the different values of l. This defines the shape of the orbitals.
I Angular Momentum Quantum Number
____discovered a simple formula relating the four lines to integers. ____advanced this formula(R_H is called the Rydberg constant) _____explained why this mathematical relationship works R_H= 1.096776x10^7 m^-1
Johann Balmer(1885) discovered a simple formula relating the four lines to integers. Johannes Rydberg advanced this formula(R_H is called the Rydberg constant) Neils Bohr explained why this mathematical relationship works RH = 1.096776 ×107 m-1
_____ tend to form cations
Metals (think metal cat collar)
what are some properties of metals?
Metals are shiny, malleable, good conducters of heat and electricity
Compare both the numbers of protons and electrons present in each to rank the following ions in order of increasing radius: As3-, Br-, K+, Mg2+.
Mg2+< K+< Br-<As3-
The magnetic quantum number describes the three-dimensional orientation of the orbital. Allowed values of ml are integers ranging from −l to l including 0: −l ≤ ml ≤ l Therefore, on any given energy level, there can be up to 1 s orbital, 3 p orbitals, 5 d orbitals, 7 f orbitals, and so forth.
Ml magnetic Quantum Number
what does the Pauli Exclusion Principle say?
No two electrons in the same atom can have the same set of four quantum numbers.
_____tend to form anions
Non metals (no metal in anions)
what are Oxyanions
Oxyanions are polyatomic ions that contain one or more oxygen atoms.
define periodic law:
Periodic Law: The properties of the elements are periodic functions of their atomic numbers.
what are polytomic ions
Polyatomic ions are electrically charged molecules (a group of bonded atoms with an overall charge).
Based on their positions in the periodic table, predict which has the largest atomic radius: Li, Rb, N, F, I.
Rb
Name how many the following electrons subshells can have s= 2 p= 6 d= 5 f= 7 take original and multiply by two to get the max electron count s=1 x 2 -> max electrons=2 p=3 x2 -> max electrons=6 d=5 x2 -> max electrons=10 f=7 x2 ->max electrons=14
Review this!
give the electron configuration of: Sm 3+
Sm3+: 1s22s22p63s23p64s23d104p65s24d105p64f5
Solving the wave equation gives a set of wave functions, or________, and their corresponding energies. Each orbital describes a spatial distribution of electron density.
Solving the wave equation gives a set of wave functions, or orbitals, and their corresponding energies. Each orbital describes a spatial distribution of electron density.
What principle says?: No two electrons in the same atom can have the same set of four quantum numbers. Therefore, no two electrons in the same atom can have the exact same energy. This means that every electron in an atom must differ by at least one of the four quantum number values: n, l, ml, and ms.
The Pauli Exclusion principle says: No two electrons in the same atom can have the same set of four quantum numbers. Therefore, no two electrons in the same atom can have the exact same energy. This means that every electron in an atom must differ by at least one of the four quantum number values: n, l, ml, and ms.
The ionic radii of the ions S2-, Cl-, and K+ are 184, 181, 138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.
The S2- ion has the smallest nuclear charge and attracts the electrons least strongly.
The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its _____ ionization energy (IE1).
The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy (IE1).
_______are the electrons occupying the inner shell orbitals. these include completely filled d or f sublevels
The electrons occupying the inner shell orbitals are called core electrons These include completely filled d or f sublevels.
______ are the electrons occupying the orbitals in the outermost shell (highest value of n)
The electrons occupying the orbital(s) in the outermost shell (highest value of n) are called valence electrons.
The energy required to remove the second most loosely bound electron is called the _______ionization energy (IE2).
The energy required to remove the second most loosely bound electron is called the second ionization energy (IE2).
The notation 3d^8 (read "three-d-eight") indicates eight electrons in the d subshell (i.e., l = ___) of the principal shell for which n = ___.
The notation 3d8 (read "three-d-eight") indicates eight electrons in the d subshell (i.e., l = 2) of the principal shell for which n = 3.
The atomic radius of main group elements generally increases down a group because:
The principle quantum number of the valence orbitals increase
The value of l for a d orbital is __. Four of the ____ d orbitals have four lobes; the other resembles a p orbital with a doughnut around the ______.
The value of l for a d orbital is 2. Four of the five d orbitals have four lobes; the other resembles a p orbital with a doughnut around the center.
The value of l for p orbitals is __. They have ___ lobes with a ____ between them.
The value of l for p orbitals is 1. They have two lobes with a node between them.
The nature of energy
The wave nature of light does not explain how an object can glow when its temperature increases
true of false: The first three quantum numbers define the orbital and the fourth quantum number describes the intrinsic electron property called spin.
True, The first three quantum numbers define the orbital and the fourth quantum number describes the intrinsic electron property called spin.
true or false: The greater the nuclear charge, the smaller the radius in a series of isoelectronic ions and atoms.
True, The greater the nuclear charge, the smaller the radius in a series of isoelectronic ions and atoms.
true or false: As the principal quantum number, n, increases, the size of the orbital increases and the electrons spend more time farther from the nucleus.
True: As the principal quantum number, n, increases, the size of the orbital increases and the electrons spend more time farther from the nucleus.
Very___________ shapes _____ equivalent orbitals in a sublevel l = 3
Very complicated shapes Seven equivalent orbitals in a sublevel l = 3
Define Wavelength
Wavelength is the distance between two consecutive peaks or troughs in a wave SI unit is in meters(M)
Give the formula for the second ionization energy
X+(g) ⟶ X^2+(g) + e^− IE2
Does Xe or Li have a larger atomic radius
Xe because its on the right side
define wave
a wave is an oscillation or periodic movement that can transport energy from one point in space to another
write the formula c=λν
c(speed of light)(3.00×10^8 m/s) = λ(wavelength) x ν(frequency)
give the formula for the speed of light
c=λν
core electrons represent ________ gas electron configurations
core electrons represent noble gas electron configurations
abbreviate Na and tell the core and valence electrons
core: 1s^2 2s^2 2p^6 3s^1 valence: 3s^1 abrv: (Ne) 3s^1
________ is when one substance breaks down down in two or more substances
decomposition reaction is when one substance breaks down down in two or more substances ex. C=A+B
aq=
dissolve in aqueous (water) soluion
l=standard positive integers and ml= minus and standard negative and positive integers
ex. n=4. l= 1, 2, 3, 4 ml= -4, -3, -2, -1, 0, 1, 2, 3, 4 ms= +1/2 or -1/2 *l cannot equal a negative number* *if l=0 then ml=0*
Any higher energy is called an________state
excited
(g) =
gas
Electrons in the lowest energy state are in the_______ state?
ground
what group are the pnictogens?
group 15
what group are the chalogens
group 16
what groups are the halogens?
group 17
what group are the noble gases
group 18
what group are the alkali metals?
group one (except hydrogen)
what metals are the alkali earth metals?
group two
triangle=
heating
if l=0 then ml=?
if l=0 then ml has to = 0
what is the agular quantum number
l
what letter represents the orbital type;:
l
l=
liquid
what are some properties of non metals
non metals appear dull and are poor conducters of heat and electricity
The term that assumes energy comes in packets called:
quanta (singular: quantum)
Tell the relationship of wavelength and frequency
short-wavelength = higher frequency & longer wavelength = low frequency
how many valence electrons does sulfur have?
six, because its in group 6!
what groups are the inner transition metals:
the last two rows, lanthanides and actinides
where are the inner transition metals
the last two separated rows!
name three examples of metals
the majority of the periodic table, Li, Be, any of the last two rows etc
what are some properties of metalloids?
they conduct heat and electricity moderatly well and possess some properties some properties of some properties of nonmetals
formula for the transition from one energy level to another:
triangle E= Ef-Ei= (-2.18 x 10^-18 J) (1/n2f - 1/n2j)
true or false: The energy of atomic orbitals increases as the principal quantum number n increases
true, the energy of atomic orbitals increases as the principal quantum n increases
true or false: to determine the number of electron configuration for an atom we add a number of electrons equal to its atomic number
true, to determine the number of electron configuration for an atom we add a number of electrons equal to its atomic number
how many valence electrons in hydrogen?
two, this one is special but you look at heliums valence electrons and theyr'e are two
how many orbitals can the d subshell have?
up to 5
how many orbitals can the f subshell have?
up to 7
how many orbitals can the s subshell have
up to one (0)
how many orbitals can the p subshell have?
up to three
write the formula of wavelength
λ=c/f λ-wavelength c-speed of light (3.0x10^8 m/s) f-frequency
The value for l for s orbitals is__ They are _________ in shape The ______ of the sphere increases with the value of _
❖The value of l for s orbitals is 0. ❖They are spherical in shape. ❖The radius of the sphere increases with the value of n.