Quiz 7 Warner
How many valence electrons do alkali metals have?
1
Which element would you expect to have the lowest first ionization energy in this part of the periodic table?
Al
Which of the following is the correct order of increasing size of atomic radii?
Al<Ga<In
_________ earth metals are elements in group 2 of the periodic table.
Alkaline
Which of the following has the largest atomic radius?
B
The largest atom in the sixth period is _____.
Cesium
P, Al, Cl, Si, Na, S, Mg Which of the elements above is the most electronegative?
Cl
Which of the following has the smallest atomic radius?
F
Which of the following elements has the lowest ionization energy?
K
The table above represents part of the second period of the periodic table, with each element placed below its atomic number. Which element out of these is the least electronegative?
Li
A more stable electronic configuration shows:
More ionization energy will be required to remove an electron
Among the following, which element of the third period has the largest atomic radius?
Na
____ _____are nonreactive, nonmetallic elements in group 18 of the periodic table.
Noble gases
Arrange the following atoms in order of decreasing atomic radius:
Rb, Sr, Sn, Ge, P
_____ has the largest atomic radius.
Rubidium
Out of Sb, Bi, Md and Tm, _____ has the smallest atomic size and _____ has the largest atomic size.
Sb, Md
Which of the following elements has the lowest electronegativity value?
Si
Arrange the following atoms in order of decreasing atomic radius: Ga, As, Sn, Sb, Te
Sn, Sb, Te, Ga, As
Which of the following explains why ionization energy decreases down a group?
The atomic radius increases, so electrons are farther from the nucleus
Which of the following is true?
The electronegativity of calcium is lower than gallium
In the periodic table, the element with the largest atomic radii is found in:
The lower left
Which electron is the first to be removed from any atom?
a valence electron
Which alkaline earth metal is used as a contrast agent for x-rays of the digestive tract?
barium
The Pauling scale of electronegativity was based on:
bond energy
Which halogen is a dark orange liquid?
bromine
Atomic size increases across a period.
false
Nonmetals have low electronegativity value.
false
Nuclear charge decreases as the atomic number increases.
false
The atomic radius of carbon is 140 pm.
false
The atomic radius of lithium is smaller than beryllium.
false
With an increase in the nuclear charge, the force of attraction between the nucleus and the outer-most electrons decreases.
false
Nitrogen has a lower ionization energy value than _____ when moving from beryllium to neon.
fluorine
Noble gases are almost completely _______ because they have eight valence electrons.
nonreactive
If "n" stands for a given principal energy level, what is the outer electron configuration of the alkaline earth metals?
ns2
If "n" stands for a given principal energy level, what is the outer electron configuration of the halogens?
ns2np5
Cesium has a greater atomic radius than lithium.
true
The effective nuclear charge and the atomic size help explain the trend of ionization energy of atoms in a periodic table.
true
The picometer is the unit used to measure atomic radii.
true
Which statement(s) are TRUE about noble gas compounds?
- Only helium and neon have not formed compounds. - Only larger noble gases can form compounds.
The difference between the second and the third ionization energies of oxygen is _____.
1,910 kJ/mol
What will be the atomic radius of copper, if the distance between two adjacent copper atoms in metallic copper is 256 pm?
128 pm
The atomic radius of a nitrogen atom is 70 pm. What is the distance between the nuclei of two bonded nitrogen atoms in a N2N2 molecule?
140 pm
Which of the following is the electron configuration for a lithium atom?
1s2 2s1
The approximate electronegativity value of the most electronegative element on the Pauling scale is _____.
4
How many valence electrons do all halogens have?
7
Which of the following is the atomic radius of chlorine if the internuclear distance between two chlorine atoms is 198 pm?
99 pm
Elements A, B and C have following relations. B is in the same group as A and B's period number is larger than A's. C is in the same period as B and C's atomic number is less than B's. The relation of their atomic radii is:
A < B < C
When an element of very low ionization potential is allowed to react with an element of very high electron affinity, _____ is obtained.
A strong ionic bond
Element A is a good conductor of heat and electricity. A has strong reducibility and can form compounds with O only by 1:1. A is:
Alkaline earth metal
Element A is metallic and locates in the Group 1 on the periodic table. Element B has one more electron than A. B is a(n)
Alkaline earth metal
Which of the following is not an alkali metal?
Aluminum
How are most ions formed?
An atom transfers electrons to or from another atom or molecule.
Which of the following orders these elements by increasing ionization energy?
Ba, Ca, As, P, Cl
Which element has the greatest first ionization energy in this part of the periodic table?
Be
Which member of the alkaline earth metals has the highest electronegativity?
Be
The atomic radius of aluminum is greater than _____.
Boron
Which of the following is larger in atomic size?
Boron
Arrange the following atoms in order of the diagram of atomic radius above:
Br, Ge, Sn, Sr
Which of the following elements has the largest atomic radius?
Ca
Atomic radius ___ across a period.
Decreases
In the periodic table, moving right from tantalum (Ta) to mercury (Hg), the atomic radii:
Decreases
Which diagram shows the relation between the atomic numbers (Z) and the atomic radius (r) of elements in the same period?
Diagonal straight line going down
The attraction that an atom exerts on a pair of electrons which are being shared with another atom for the formation of covalent bonds is referred to as its _____.
Electronegativity
When _____ is measured on the Pauling scale, it gives a quantity which is/has _____.
Electronegativity, dimensionless
The table above represents a small piece of the periodic table with each element represented by it's symbol and atomic number. Which element here has the greatest electronegativity?
F
Which member of the halogen elements has the highest electronegativity?
F
Which ionization energy of the following has the greatest value?
First ionization energy (Si → Si+)
The covalent radius of bromine is:
Half the Br-Br bond length
Which group/family contains elements with the smallest radius within the same period?
Halogens
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 member of the alkali metals has the highest electronegativity?
Li
Which of the following elements has the largest ionization energy?
Li
Considering the second period elements, which of the following has the largest atomic radius?
Lithium
The _____ electronegativity of metals and _____ electronegativity of non-metals means the reaction is most favorable between a metal and a non-metal.
Low, High
Which of the following has the largest atomic radius?
Na
A is an alkaline earth metal. If A loses two electrons to gain a complete octet, it has the same number of electrons as a(n)
Noble gas
Which statement best explains the reactivity of noble gases?
Noble gases are typically unreactive since they have full outer electron shells.
In general, as an approximation, elements with an electronegativity value of 2.0 or greater are _____.
Nonmetals
Which of the following elements will have the highest electronegativity?
O
Which list of elements from Period 2 is arranged from highest to lowest ionization energy?
O, N, B
The atomic size of silicon is greater than _____.
Phosphorus
Which of the following has the largest atomic radius among Group 16 elements?
Po
Electronegativity decreases from top to bottom within a respective group as:
Proceeding down the group, the size of atoms increases so the effective nuclear charge decreases on the electrons
Which of the following best explains why atomic radius decreases left to right across a period?
Protons are added to the nucleus, and the force of attraction on electrons is stronger
Which member of the alkaline earth metals has the smallest electronegativity?
Ra
Which of the following is the correct order of the increasing size of atomic radii?
Si<Sn<Pb
The atomic radii of oxygen and fluorine are _____ nitrogen.
Smaller than
When moving from left to right across a period,the outer electrons feel a _____ attraction towards the nucleus and the atomic radius _____.
Stronger, decreases
Why is atomic radius not a well-defined quantity?
The boundary of an electron cloud is not distinct.
Which of the following explains why electronegativity decreases from right to left across a period?
The number of protons decreases, so the nucleus is less positively charged
How does the principal energy level and the nuclear charge of an atom change in going from left to right across a period?
The principal energy level stays the same and the nuclear charge increases.
If two bonded atoms have the same electronegativity:
The shared pair of electrons will lie exactly in the center
During most chemical reactions, what happens to the atoms of a halogen?
They gain one electron.
Which group has the lowest electronegativities?
alkali metals
Which of following has the lowest value of ionization energy?
alkali metals
Which other elements of the periodic table do halogens readily react with to form halide salts?
alkali metals and alkaline earth metals
Ionization energy depends upon:
all of the above
Which of the following is/are true?
all of the above
Which element has a larger atomic radius than phosphorus?
aluminum
Negatively charged ions are called _____.
anion
Where are halogens frequently found in nature?
as salts in the ocean
Which alkaline earth metal is used as a white pigment in paints and toothpaste?
calcium
Positively charged ions are called _____.
cation
Atomic radii _____ while moving from scandium to chromium.
decrease
Atomic radius generally _____ from left to right across a period 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
horizontal diagram In the diagram of elements above, which of the following describes the change of atomic radius along the direction of the arrow?
decreases
The reactivity of a given element is most closely related to its _____.
electron configuration
Among halogens, chlorine is the most electronegative element.
false
An effective nuclear charge is the charge actually felt by the outer electrons and is 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
Atomic radii in transition metals follow a systematic order while moving from left to right.
false
Atomic radii increase in size with an increase in the atomic number across a period.
false
Electron affinity and electronegativity are both measured in energy units.
false
Electronegativity generally increases while moving from top to bottom in the periodic table.
false
Electronegativity increases as you move from aluminum to thallium down the group 13 elements.
false
Electronegativity is directly related to the metallic properties of elements.
false
Group 1A elements have two electrons in their outer shell.
false
Hydrogen is considered to be an alkali metal.
false
Ionization energy is expressed in the units of electron volts per atom.
false
Ions form because the loss of one or more electrons makes them less stable than their corresponding atoms; this state requires more energy to maintain.
false
The atomic radius tends to increase as progression is made across a period from left to right.
false
The atomic size of beryllium is larger than lithium.
false
The attraction between the nucleus and electrons increases while moving down a group in the periodic table.
false
The electronegativity value is lowest in polonium when we move from left to right in the sixth period.
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 of 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 number of valence electrons present in alkali metals are 2.
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 outer most electrons from those atoms which have many electrons. Therefore ionization energy will increase while moving down a group.
false
The size of an atom is independent of the number of protons in the nucleus, the number of energy levels holding electrons, and the number of electrons in the outer energy level.
false
There is no difference between electron affinity and electronegativity.
false
True or False: Among all halogens, fluorine has the smallest electronegativity
false
True or False: At room temperature and 1 atm, all gases are diatomic molecules.
false
True or False: Atomic radius increases down a group because the the number ofvalence electrons increase with increasing electrons.
false
True or False: Cl, Pb, Sn, Ar, Se, Br The order of increasing atomic radius of all atoms above is:
false
True or False: In Group 16, S has the smallest atomic radius.
false
True or False: Ionization energy increases down a group because the number of protons increases and it's more difficult to lose electrons.
false
When a graph is plotted between atomic radii versus the number of protons for the first transition metal series, a straight line is formed.
false
When moving from antimony to iodine, the first ionization energy value decreases.
false
When moving from gold to lead, the atomic radius increases.
false
When we move from boron to carbon, atomic size increases.
false
While moving across the periodic table from left to right there is an increase in atomic radius. .
false
While moving from aluminum to thallium, gallium has an electronegativity value lower than indium.
false
Arrow directions represent increasing trend of ionization energy. Which of the following correctly shows the general trend?
first arrow is vertical going up and second is horizontal going right
The element _____ is assigned the highest electronegativity, with a value of ____.
fluorine; 4.0
Which diagram shows the relation between the atomic numbers (Z) and the atomic radius (r) of elements in the same group?
graph with diagonal straight line going up
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
Where are the alkali metals located in the periodic table?
group 1
Halogens are located in what group on the periodic table?
group 17
Alkaline earth metals are located in what group on the periodic table?
group 2
Where are the alkaline earth metals located in the periodic table?
group 2
Element A is located between group 16 and noble gas on the periodic table. A is a(n)
halogen
Which group has the highest electronegativities?
halogens
Across a period, the effective nuclear charge increases and therefore it becomes _____ to remove an electron.
harder
In the following elements, _____ has the highest ionization energy.
helium
As the number of valence electrons increases, the electronegativity value becomes _____.
higher
What gas is produced when an alkali metal reacts with water?
hydrogen only
Ionization energy generally _____ from left to right across a period of the periodic table.
increases
The electronegativity value _____ when one moves from beryllium to nitrogen.
increases
Upon moving down in a group, the distance between the valence electrons and the nucleus _____.
increases
When moving down a group,the atomic size _____ and therefore the ionization energy decreases.
increases
vertical diagram In the diagram of elements above, which of the following describes the change of atomic radius along the direction of the arrow?
increases
Which halogen is a purple-gray solid?
iodine
Which of the following halogens has the largest atomic radius?
iodine
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
Compared with alkali metals, the alkaline earth metal in the same period has ___ electronegativity.
larger
In alkali metals, the atomic radius of potassium is greater than _____.
lithium
What would be the name for Li+?
lithium ion
When a group 1 element reacts it
loses one electron.
Metals tend to have generally _____ electronegativities, while nonmetals tend to have generally _____ electronegativities.
low; high
Elements in the alkaline earth metal family of the periodic table have ________ electronegativity values than elements in the halogen family of the periodic table.
lower
Which alkaline earth metal is found in flares?
magnesium
P, F, Cl, Si, C, O, Mg Which of the elements above is the least electronegative?
mg
The second ionization energy is greater than the first because it's ___ to remove an electron from a cation.
more difficult
Which of the following has the highest ionization energy?
neon
Which of the following characteristics of halogens is not correct?
none of the above
If "n" stands for a given principal energy level, what is the outer electron configuration of the noble gases (except He)?
ns2np6
The ______ rule is based on the number of electrons in the noble gases, which are the least reactive elements.
octet
_________ proposed the first scale of electronegativity.
pauling
Complete the sentence using one of the following terms: s, p, d, or f. Alkali metals are a part of the ____ block of the periodic table.
s
Complete the sentence using one of the following terms: s, p, d, or f. Alkaline earth metals are a part of the ____ block of the periodic table.
s
The presence of inner-shell electrons cause the outermost electrons of an atom to be less attracted to the nucleus. This is called electron _____.
shielding
_____ has the smallest atomic radius.
silicon
Compared with halogens, the alkali metal in the same period has ___ electronegativity.
smaller
Which of the following elements has the lowest ionization energy?
sodium
Which of the following is not a Group 2A element?
sodium
Which alkaline earth metal is used in red fireworks?
strontium
Which element has the highest first ionization energy?
sulfur
Compared to the atomic radius of a carbon atom, the atomic radius of a silicon atom is larger because of an increase in:
the number of principal energy levels
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
Atomic radii decrease while moving left to right across the periodic table.
true
By having knowledge of the atomic radius of an atom, the size of the atom can be measured.
true
Cesium is considered the most electropositive stable element.
true
Cesium is the most electropositive stable element of all the alkali metals.
true
Chlorine has a larger atomic radius than fluorine.
true
Group 1A elements are highly reactive.
true
Group 2A elements are moderately hard.
true
In the second period, the atomic radii decrease as one moves from lithium to neon.
true
Metalloids have electronegativity values close to 2 (on the Pauling scale).
true
Moving across a period from left to right increases the ionization energy.
true
Non-metallic elements have high electronegativity.
true
The ability of an atom in a molecule to attract shared electrons is called electronegativity.
true
The alkali metals, which are at the extreme left of the periodic table, have the largest size in the periodic table.
true
The atomic radius of xenon is greater than helium.
true
The atomic size is the distance from the nucleus to its outermost shell of electrons.
true
The attractive force between the outer-most electrons and the nucleus of an atom is inversely proportional to the distance between them.
true
The elements of Group 1A have the largest atomic radii in their periods.
true
The first ionization energy values of Zn, Cd, and Hg are relatively higher than their immediate neighbors.
true
The size of atomic radii within a group of elements increase while moving from top to bottom.
true
The tendency of an atom to attract the shared pair of electrons towards itself in a covalent bond is known as electronegativity.
true
True or False: A is a metal in the same group as Na, so A is an alkali metal.
true
True or False: Astatine is located in group 17 so it is considered a halogen element.
true
True or False: Cesium is an alkali metal.
true
True or False: Ionization energy increases across a period, because it's more difficult to lose electrons as the number of protons increase.
true
Ways in which ions may form include ______.
two of the above
Which describes the state that the noble gases are found at room temperature?
unreactive monatomic gases
Chemical bonds involve the transfer or sharing of _____.
valence electrons only
With which noble gas was the first noble gas compound finally formed?
xenon
