Chem periodic trend
Arrow directions represent increasing trend of electron affinity.Which of the following correctly shows the general trend?
(vertical: up and down) GOING UP ^ (horizontal: side to side) TO THE RIGHT ->
Arrow directions represent increasing trend of ionization energy. Which of the following correctly shows. the general trend.
(vertical: up and down) GOING UP ^ (horizontal: side to side) TO THE RIGHT ->
How many electrons must be added to a fluorine atom to achieve the electron configuration of a noble gas?
1
Abridged Periodic Table: B C 1 2 3 4 5 6 7 S Cl 8 Each number represents an elements.Which of the following lost contains the three elements with the highest electron affinities?
1, 2, 3
The difference between the second and the third ionization energies of oxygen is. _________.
1,910 kJ/mol
The electron affinity for Be and Mg is almost zero since:
2s and 3s orbitals in Be and Mg respectively are completely filled
Abridged Periodic Table: 1 Be 2 C N 3 Na 4 Al 5 P S Each number represents an element. Which one of them has the highest electron affinity?
3
Abridged Periodic Table: Li 1 2 C N 3 Mg Al 4 5 Each number represents an elements. Which number has the smallest electron affinity?
3
Use the periodic table above ti answer the following question. Which element releases the most energy after gaining an electrons to become an anion?
3
Abridged periodic table: Li 1 2 3 4 5 Mg Al Si P Each number represents an elements. Which two of them have the highest electron affinity?
3,4
"Here is a small piece of the periodic table which shows the first two groups with their element symbols and atomic numbers" Group I Group 2 Li-3. Be-4 Na-11. Mg-12 K-19. Ca-20 Rb-37. Sr-38 cs-55. Ba-56 Which element has the greatest first ionization energy in this periodic table?
4, Be, beryllium (any of these)
"Here is a small piece of the periodic table which shows a small number of the elements in groups 13-18 with their element symbols and atomic numbers." Which element has the lowest first ionization energy in this part of the table?
Al
Which of the following has the lowest value of ionization energy?
Alkali metals
Which of the following is/are true?
All of the above
How are most ions formed?
An atom transfers electrons to or from another atom or molecule
Which of the following elements has the smallest electron affinity?
Ar
Which of the following orders these elements by increasing ionization energy?
Ba, Ca, As, P, Cl
Which alkaline earth metal has the highest electron affinity?
Be
K, Cl, Ar, P, Rb Which of the following orders the elements above by decreasing electron affinity?
Cl, P, K, Rb, Ar
Order these elements by dressing electron affinity: Na, Al, S, K, F
F, Sl, Al, Na, K
Across a period, ionization energy continually increases with no exceptions
FALSE
An effective nuclear charge is the charge actually felt by the outer electrons its more than the actual nuclear charge
FALSE
An ion always has the same number of protons and electrons
FALSE
As the size of an atom increases, the energy required to remove the outermost electron also increases.
FALSE
Density is a physical property that does not exhibit periodicity.
FALSE
Ionization energy increases down a group because the number of protons increases and it's more difficult to lose electrons.
FALSE
Ionization energy is expressed in the units of electron volts per atom
FALSE
P has a lower ionization than S because its 3p electrons are all unpaired
FALSE
The 3p electrons in Si can shield the 3s electrons
FALSE
The first ionization energy of hydrogen is greater than that of helium
FALSE
The first ionization energy of rubidium is higher than that of sodium
FALSE
The first ionization energy silicon is less than the first ionization energy of aluminum
FALSE
The force of attraction between the nucleus and an electron decreases with an increase in nuclear charge
FALSE
The ionization energy generally increases down the group
FALSE
The larger the value of ionization energy, the easier it is to remove an electron from an atom
FALSE
The outer electrons shield the inner electrons from the positive charge of the nucleus.
FALSE
The shielding effect makes it easier to remove the outermost electrons form those atoms which have many electrons. Therefore ionization energy will increase while moving down a group.
FALSE
When moving from antimony to iodine, the first ionization energy value decreases.
FALSE
With an increase in the nuclear charge, the force of attraction between the nucleus and the outermost electrons decreases.
FALSE
ionization energy increases down a group because the number of protons increases and it's more difficult to lose electrons
FALSE
Among all the halogens, which one has the highest electron affinity?
Flourine
Which group has the highest electron affinity within a period?
Halogens
Bromine has more electron affinity than _________
Iodine
What happens to an atom when it gains electrons?
It becomes a negatively charged ion
What happens to an atom when it loses electrons?
It becomes a positively charged ion
Which of the following elements has the lowest ionization energy?
K
Order these elements by increasing electrons affinity: K, Se, S, F
K, Se, S, F
Which of the following elements has the largest ionization energy?
Li
Which of the following anions is least likely to occur
Na -
Which of the following elements has zero electron affinity?
Neon
In a period, which kind of element is least likely to form monovalent anion?
Noble gas
Among the following, which posses the highest electron affinity?
Non-metals
The electron affinity of the members in the oxygen family follows the order_________
O > S > Se
Which list of elements from Period 2 is arranged from highest to lowest ionization energy?
O, N, B
Which statement about electrons shielding is FALSE?
Outer electrons significantly shield inner core electrons, canceling out some of the inner electrons' charge
A nitrogen atom has 3 unpaired electrons, while an oxygenated has 2 unpaired electrons?
TRUE
An effective nuclear charge is the charge experienced by a specific electron within an atom
TRUE
An increase in the number of electrons in an atom will result in a decrease in the ionization energy
TRUE
Ionization energy increases across a period because it's more difficult to lose electrons as the number of protons increase
TRUE
The attractive force between the outer-most electrons and the nucleus of an atom inversely proportional to the distance between them
TRUE
The effective nuclear charge and the atomic size help explain the trend of ionization energy of atoms in a periodic table
TRUE
The first ionization energy for Ni is slightly less than that for Co because Ni has one more 3d electron to provide shielding.
TRUE
The first ionization energy values of Zn, Cd, and Hg are relatively higher than their immediate neighbors
TRUE
moving across a period from left to right increase the ionization energy.
TRUE
Which of the following explains why ionization energy decreases down a group?
The atomic atrium increases, so electrons are farther from the nucleus
Why is the ionization energy of oxygen lower than the ionization energy of nitrogen?
The electron to be removed from the oxygen atom is slightly repelled by another electron in the same orbital
Which electrons is the first to be removed from any atom?
a valence electron
Ionization energy depends upon:
all of the above
The 3p electron in an aluminum atom is shielded by:
all of the other electrons in the atom
negatively charged ions are called _________
anions
positively charged ions are called _________
cations
In general electron affinity_________ from top to bottom down a group. of the periodic table.
decreases
Ionization energy generally _________ from top to bottom down a group of the periodic table.
decreases
When moving from the third period to the seventh period , ionization value _________.
decreases
Which is correct?
electrons in an s sub level can shield the p electrons that are in the same principal energy level
Which ionization energy of the following has the greatest value?
first ionization energy (Si -> Si+)
Nitrogen has a lower ionization energy value than _________ when moving from beryllium to neon.
fluorine
The first ionization energy of sodium is _________ than potassium
greater
Compared to the ionization energy of a lithium atom, the ionization energy of a beryllium atom is larger. This is primarily a result of the beryllium atom having:
greater nuclear charge
Across a period, the effective nuclear charge increases and therefore it becomes _________ to remove an electrons
harder
in the following elements, _________ has the highest ionization energy
helium
In the periodic table, the halogens possess the/a _________ electron affinity
highest
The electron affinity of _________ is higher than lithium.
hydrogen
In general electron affinity _________ from left to right across a period of the periodic table.
increases
Ionization energy generally _________ from left to right across a period of the periodic table
increases
When moving down a group, the atomic size _________ and therefore the ionization energy decreases
increases
If an atom gains or loses electrons, it becomes a(n)
ion
Compared to the ionization energy of a magnesium atom, the ionization energy of a calcium atom is smaller, This is primarily because the calcium atom:
is larger than the magnesium atom
Which of the following elements has the highest electrons affinity?
lithium
What would be the name for Li+
lithium ion
When a group 1 elements reacts it _________
loses one electrons
The second ionization energy is greater than the first because it's _________ to remove an electron form a cation
more difficult
A more stable electron configuration shows:
more ionization energy will be required to remove an electron
Which of the following had the highest ionization energy
neon?
Electron affinity is the amount of energy when an extra electron is added to a neutral gaseous atom.
release
The presence of inner-shell electrons causes the outermost electrons of an atom to be less attracted to the nucleus. This is called electron _________
shielding
Which of the following elements has the lowest ionization energy?
sodium
Which element has the highest first ionization energy?
sulfur
A single 3s electron in a magnesium atom is shielded by:
the 1s, 2s and 2p electrons
Ways in which ions may form include _________
two of the above
