Chem - Electron Configuration and Periodic Table Test
"power" on periodic table is based off of (trend for this in groups and periods)
# of valence electrons and # of energy levels; the more valence electrons you have with the least amount of energy levels is better moving down groups = less powerful // less powerful when giving electrons moving across period = more powerful // more powerful when taking electrons (Flourine = big boss)
first ionization energy (what it is, how high is it and why)
the energy required to remove the first valence electron from an atom; not very high bc its the first one
third ionization energy (what it is, what it is required for, how high is it)
the energy required to remove the third valence electron; Required to remove an electron with +2 charge; immensly high
What is the total number of valence electrons in an atom of boron in the ground state? 1, 7, 3, 5
3
What is the total number of valence electrons in an atom of xenon, XE? 0, 2, 8, 18
8
Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having? A larger nuclear charge, a smaller nuclear charge, more principal energy levels, fewer principal energy levels
A larger nuclear charge
Which element in period 5 of the periodic table is a transition element? Sr, Sb, Ag, Xe
Ag
Which has an electron configuration ending in s2p1: Na, Tl, Al
Al
Which sequence of elements is arranged in order of decreasing atomic radii? Al, Si, P // Li, Na, K // Cl, Br, L // N, C, B
Al, Si, P
Transition Metals (Groups 3-12)
All the d block groups on the periodic table; filled as core electrons, not valence electrons
Pauli Exclusion Principle
An atomic orbital may describe at most two electrons, each with opposite spin direction
Which has the smallest ionization energy: N, P, As
As
noble gases (how many valence electrons they have, highest what (3 things), smallest what (1 thing)
Atoms that have eight electrons in their outermost energy level; highest ionization energy, electronegativity, affinity, and smallest atomic radius
which of the following group 2 elements has the lowest first ionization energy? Be, Mg, Ca, Ba
Ba
Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? Be, Mg, Ca // Ca, Mg, Be // Ba, Ra, Sr // Sr, Ra, Ba
Be, Mg, Ca
Which is a member of the halogen family: S, Cl, Ar
Cl
halogens (what it contains, how many valence electrons it has, how reactive they are)
Contains nonmetals; 7 valence electrons in it's outermost energy level; Very reactive
valence electrons
Electrons on the outermost energy level of an atom
family/group
Elements in the same vertical column of the periodic table
The group 17 element with the highest electronegativity is? Flourine, Chlorine, Bromine, Iodine
Flourine
Why does fluorine have a higher ionization energy than iodine?
Fluorine has a higher ionization energy because it is in a lower energy level (less shielding effect) so Fluorine has a stronger nuclear force on the surrounding electrons and require more energy to remove electrons
Which has the largest atomic radius: Ga, Al, Si
Ga
Which has 4 energy levels: Si, Ge, Sn
Ge
alkali metals
Group 1
alkaline earth metals
Group 2
Which is a nonmetal: H, Li, Na
H
Which noble gas has the highest first ionization energy? Radon, Krypton, Neon, Helium
Helium
Which is a transition metal: Hg, Tl, Pb
Hg
Which Group 17 element has the least attraction for electrons? F, Cl, Br, I
I
which element is a member of the halogen family K, B, I, S
I
Which sequence correctly places the elements in order of increasing ionization energy? H --> Li --> Na --> K I --> Br --> Cl --> F O --> S --> Se --> Te H --> Be --> Al --> Ga
I --> Br --> Cl --> F
Which of the following atoms has the largest atomic radius? Na, K, Mg, Ca
K
Which is an alkali metal: Li, Be, B
Li
which is a metal: Li, Si, S
Li
Which is a gas at room temp: B, C, N
N
Which element in Group 16 has the greatest tendency to gain electrons? Te, Se, S, O
O
Which has the greatest electron affinity: Al, Si, P
P
which is a metalloid: Pb, Bi, Po
Po
which has the largest atomic mass: K, Ca, Sc
Sc
Which has 6 valence electrons: As, Se, Br
Se
Which has the largest atomic number: V, Nb, Ta
Ta
core electrons (where they are, what they're not involved in)
The electrons in the inner shells of an atom; these electrons are not involved in forming bonds
second ionization energy (what it is, how high is it and why)
The energy needed to knock off the second valence electron; higher than first because it is disturbing the previous configuration
Which statement best describes group 2 elements as they are considered in order from top to bottom of the periodic table? The number of principal energy levels increases, and the number of valence electrons increases The number of principal energy levels increases, and the number of valence electrons remains the same The number of principal energy levels remains the same, and the number of valence electrons increases The number of principal energy levels remains the same, and the number of valence electrons decreases
The number of principal energy levels increases, and the number of valence electrons remains the same
As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare? The relative electronegativity decreases, and the atomic radius decreases The relative electronegativity decreases, and the atomic radius increases The relative electronegativity increases, and the atomic radius decreases The relative electronegativity increases, and the atomic radius increases
The relative electronegativity increases, and the atomic radius decreases
Which has an electron configuration ending in s2d2: Ca, Sc, Ti
Ti
Which is a noble gas: Te, I, Xe
Xe
affinity
ability of an atom to accept an electron
Why does electronegativity increase across a period?
atomic number increases and number of electrons stays the same so the protons are basically stronger causing more electrons to be attracted to said element
octet rule (what it is, what is formed using this)
atoms react by gaining or losing electrons to acquire the stable electron structure of usually eight valence electrons; ionic compounds are created bc of this
Coulumbic attraction // how it affects atomic radius and electronegativity and ionization energy // family/group trends for decreasing coulombic attraction
attraction btwn positively and negatively charged particles (protons and neutrons); if there are more electrons with less energy levels in between them and the nucleus coulombic attraction will be higher causing atomic radius to shrink and electronegativity and ionization energy to increase
metalloid behavior/properties
can show both, metal, or non metallic properties (it depends on who is next to them)
As metallic properties in an element increases, its ionization energy...
decreases
As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally... decreases, increases, stays the same
decreases
Why does ionization energy decrease as you go down a group?
electrons are farther from the nucleus making it easier to remove from the atom (low coulombic attraction)
the amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as... First ionization energy, activation energy, conductivity, electronegativity
first ionization energy
which properties are most common in nonmetals? low ionization energy and low electronegativity low ionization energy and high electronegativity high ionization energy and low electronegativity high ionization energy and high electronegativity
high ionization energy and high electronegativity; bc nonmetals are very strong
period
horizontal row in the periodic table
octet rule exceptions (how many valence electron hydrogen, beryllium, and boron wants)
hydrogen wants 2; beryllium wants 4; boron wants 6
metallic properties
increase as you move down a group bc less attraction between nucleus and electrons bc of increasing number of energy levels and subshells
As each successive element in group 15 of the periodic table is considered in order of increasing atomic number, the atomic radius? decreases, increases, remains the same
increases bc of more energy levels
family/group trends for increasing electronegativity, ionization energy, and affinity (why)
increases from down to up bc # of electrons is decreasing whilst # of energy levels is too
period trends for increasing electronegativity, ionization energy, and affinity
increases from left to right
period trends for increasing ionic radius
increases from left to right
period trends for increasing atomic radius and reactivity (why)
increases from right to left radius bc of coulombic attraction and reactivity bc the elements on the left have less electrons to lose than those on the right do
family/group trends for increasing ionic radius
increases from up to down (as electrons are being taken)
family/group trends for increasing atomic radius and why
increases from up to down (bc of more energy levels)
As the elements of Group 1 on the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases bc of... Decreasing radius and decreasing shielding effect Decreasing radius and increasing shielding effect increasing radius and decreasing shielding effect increasing radius and increasing shielding effect
increasing radius and increasing shielding effect
The strength of an atom's attraction for the electrons in an atomic bond in the atom's... electronegativity, ionization energy, heat of reaction, heat of formation
ionization energy
the ability of carbon to attract electrons is ? greater than that of nitrogen, but less than that of oxygen less that that of nitrogen, but greater than that of oxygen greater than that of nitrogen and oxygen less than that of nitrogen and oxygen
less than that of nitrogen and oxygen
stairs on periodic table
metalloids (right above and right below)
anion and why it forms and why this makes sense (relating to how neg charges are formed)
negatively charged ion; created as a result of an element receiving/taking an electron to another element during ion formation (gaining neg charged electrons = pos. + neg. = neg.)
which of these elements has the least attraction for electrons in a chemical bond? Oxygen, flourine, nitrogen, chlorine
nitrogen
The elements calcium and strontium have similar chemical properties because they both have the same? atomic number, mass number, number of valence electrons, number of completely filled sublevels
number of valence electrons
hund's rule
orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin
ions
positively and negatively charged atoms
cation and how it forms and why this makes sense (relating to negs making pos)
positively charged ion; created as a result of an element giving an electron to another element during ion formation (losing neg charged electrons = two negs. make a pos. )
Why do elements in the same group have similar properties?
same number of valence electrons
Electronegativity
the ability of an atom of an element to attract electrons
ionization energy (what it is, what it is used for)
the energy required to remove an electron from an atom or the amount of energy atom required to become an ion (cation or anion); most likely to get nobel gas configuration
shielding effect (what is it, what does it cause an increase in and a decrease in; trends in family/group and period)
the reduction of the attractive force between a nucleus and its outer electrons due to the blocking effect of inner electrons (core electrons' interference); causes increase in atomic radius as well as decrease in coulombic attraction; increases from top to bottom and from left to right
Aufbau Principle
the rule that electrons occupy the orbitals of lowest energy first
An element with a partially filled d sublevel in the ground state is classified as? Halogen, transition metal, an alkali metal, an alkaline earth metal
transition metal
On the periodic table, all the elements within group 16 have the same number of? valence electrons, energy levels, protons, neutrons
valence electrons
periodic law
when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties