CH. 1 Atomic Structure and Periodic Trends Flashcards
Two atoms bonded together are called
molecule
2+ molecules bonded together is called
Compound
Most of the mass of an atom comes from
Protons and neutrons, protons have a mass of 1 amu
Electrons furthest from the nucleus are ______ stable and _____ in energy
Least stable; HIghest in energy
The identity of Each atom comes from
the proton amount, by changing this you would change the atom
What is a mass number?
The total number of protons and neutrons. it is represented as the top number.
What is the atomic number?
a total number of protons.
How could you determine the number of neutrons an atom has?
Subtract the atomic number (proton number) from the mass number.
When an atom changes the number of neutrons it creates a ________. When it changes the number of electrons it creates a __________.
neutrons = isotope electrons = ion
Atoms in the elemental state are said to be neutral, what does this mean?
number of protons = number of electrons
A positivley charged ion is called
Cation
A negativley charged ion is called
Anion
Which is said to be proton rich, Cation or Anion?
Cation
Columns 15 -17 typically ______ electrons.
GAin
Columns 1 & 2 typically ______ electrons.
Lose
Cations that have a lower ionic charge have the suffix ______. While those with a higher ionic charge have the suffix _______.
lower = ous higher = ic
Compare Cu+ and Cu2+ nomenclature
Cu+ = Cuporous Cu2+ = Cupric
Monoatomic Anions use the suffix ___.
-ide
hydride, oxide
What are Oxyanions?
Anions that contain Oxygen. They are diatomic molecules, as oxygen readily accepts 2 elections.
Oxyanions that contain oxygen use the suffix _____. If there is an anion that contains more oxygen the suffix _____. is used.
baseline - ite
+1 oxygen molecule =ate
(Nitrite - NO2 & Nitrate - NO3)
When comparing oxyanions, what does the prefix Per and hypo mean?
Hypo = 1 less oxygen molecule than -ite Per = 1 more oxygen than -ate.
When naming polyatomic anions with hydrogen
use terms for hydrogen before parent name.
The Bohr model is based on the ability of protons to do what?
keep attraction forces upon negatively charged electrons.
An electron shell of n= 1 would be ____ to a nucleus compared to a electron shell of n=3
closer
For an electron to move from a lower shell to a higher shell it must
Input/absorb energy in the form of a photon
For an electron to move from a higher shell to a lower shell it must
release/emit energy in the form of a photon
What is Electromagnetic Radiation
The type of energy that is absorbed or emitted when moving electrons between shells
The amount of energy of a photon is equal to (equation)?
Planks constant x frequency of light
E = h X f) (h= Planks, f = frequency of light
How do you calculate the frequency of light?
speed of light divided by wavelength
(f = C/λ) (C = speed, λ = wave)
So E = h x f is the same as E = h (C/λ)
The amount of energy emitted or absorbed can be calculated using the Rydberg formula, what is it?
ΔE =h x c/λ or ΔE= R (1/n2 (inital) - 1/n2 (final))
R = 2.18 x 10^-18
When using the Rydberg formula, if it is a negative number this means?
Energy was emitted to move to a lower shell
What is the order of the four quantum numbers?
electron shell> subsell > orbital> electron
What is a principal quantum number?
The number that specifies the shell (n = 1)
What is an Angular momentum quantum number (or Azimuthal)
This describes the shape of the orbital, or what subshell the electrons are in
What are the various Angular momentum shapes of subshells and how many electrons can they fit?
Describes the shape of the orbital. s= sphere p = dumbbell d = double dumbbell f = complex
What is the Magnetic quantum number (m sub L)
This identifies the spatial orientation of the orbital.
s orbital - 2 electrons
p orbital = 6 electrons
d orbital = 10 electrons
(each increase in subshell is equal to +& - L. L = 0 S orbital = 2 electrons. L = 1 is P sub shell and is equal to -1,0,+1 with 2 electrons for each = 6. L = 7 would be -7 to +7)
What is the last quantumm number?
Spin number (m sub s). This defines spin orientation, which could be neg or positive half spin but not the same. Paired electrons must have opposite spins.
For electron configuration, you should always predict where _____ is first before filling the _____ shells.
the lowest energy electrons higher shells (higher energy)
Electron configuration is based on
Angular momentum
Describe the graph of electron configuration
Number paper 1 - x, placing angular momentum letters in order (3s, 3p, 3d). Drawing a parallel line go from top right to bottom left
Describe the short-cut method for electron configuration
Divide the periodic table into blocks, s block first 2 columns, d block trans., p block last 6, f block bottom,. Take the noble gas of the period above atom of interest to represent electron configuration minus the valence. Using remaining electrons and block atom is found in to determine the rest of the electron configuration.
Using the short-cut method what is the electron configuration of Potassium?
[Ar]4s1
When determining an Ion configuration you should
move a space to the right for every electron added and a space to the left for every electron lost.
Electrons should always be removed from the _____ first.
subshell with the highest electron number
On a periodic table, _____ have the same number of valence electrons and share the same physical and chemical properties.
Groups/columns
Within a group/column the number of electrons _______ from top to bottom
INcreases
What are the three main categories of elements?
Metals, non-metals, metalloids
Which category of elements is said to be a good conductor of electricity, solid under normal conditions, and malleable?
Metals
Which category of elements is said to be poor electrical conductors?
non-metals
Which category of elements is said to be brittle, and a poor to decent conductor of electricity?
metalloids
Which group are the alkai metals?
Group 1 (exluding hydrogen)
Which group are the alkai earth metals
Group 2
Which group are the trans. metals?
group 3-12 (they are hard, durable, and conduct electricity)
Describe group 13
1 metalloid (Boron) rest are metals. They form +3 cations
Which group is the carbon family?
group 14. carbon = non-metal Silicon & germanium = metalloids Tin & lead = metal this group readily forms oxides
Which group is the Nitrogen family?
group 15.
Nitrogen & Phos = nonmetals
Arsenic & Antimony = metalloids
Bismuth = metal
Which group is the Chacogens?
Group 16
Oxy, Sulfur, and Selenium = nonmetal
Tellerium & Polonium = metalloids
- readily form +2 Anions
Which group is nonmetal and highly reactive to accepting 1 electron to make +1 Anion?
Group 17 Halogens
Which group is made nonmetals and unreactive due to full octet.
Group 18.
Nobel gases
Have a low boiling point
What is Z sub eff?
Effective Nuclear charge.
It is the attractive force between the positively charged protons and negatively charged valence electrons.
Which direction of the periodic table would increase the effective nuclear charge (Z sub eff)?
left to right
This is because the number of protons increases, while the shielding effect from the electrons is relatively low.
bottom to top - shielding effect is lower towards the top
Which direction of the periodic table would show a decrease in effective nuclear charge?
right to left (reduction of protons/atomic mass)
Top to bottom (shielding from electrons)
What is an atomic radius?
The radius of neutral atoms, which is related to Z sub eff
In which direction would the atomic radius decrease (make smaller)?
Left to right in a period.
This is due to the higher atomic mass which pulls the electrons closer.
bottom to top in a group
going down the periodic table increases the shell, and electron, count. This would make the radius smaller in the top.
What is the Ionic radius?
Radius of charged ions of a given atom.
The radius depends upon electrostatic repulsion (like charges repel). The higher the Anion charge the increase in radius, the higher cation the lower the radius.
What is Ionization energy?
Energy needed to remove one valence electron from a neutral atom in a gas state.
Ionization is a positive quantity because
energy is needed to move an electron further away from the nucleus (like electromagnetic radiation).
What is the relationship between the energy needed and removing electrons in an Ionization?
The first electron requires low energy than the first. Removing electrons decreases electrostatic repulsion, moving remaining electrons closer and at a more stable orbital.
In an Ionization, removing electrons from a full orbital
requires a dramatically high amount of energy due to the stability of an octet.
ionization energy increase
left to right in a period
bottom to top in a group
Ionization energy decreases
right to left in a period
top to bottom in a group
What is electron affinity?
The ability to establish an octet.
Which atoms have the highest electron affinity?
left to right (Halogens the highest)
bottom to top ( Florine the highest)
Electrons must always be removed from which subshell?
The subshell with the highest principal quantum number (remove from 4s before 3d, or work backward).
An exception to removing electrons from subshell is?
Subshells like to be stable and half-filled and fully filled are most stable.
e.g p subshell 3 or 6 electrons is most energetically favorable
Additionally transition metals love to perform this action
What is electronegativity?
the ability of an atom to attract electrons that are shared in a chemical bond between two atoms.
What is the trend for electronegativity?
Within a period atoms are more electronegative on the right than the left.
Within a column, atoms are more electronegative at the top compared to these below
