Chapter 6 Chemistry quiz
Circle the atom in each pair that has the greater electronegativity. a) Ca Ga b) Li O c) Cl S d) Br As e) Ba Sr f) O S
2,2,1,1,2,1,
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) a larger nuclear charge (more protons) B) a smaller nuclear charge C) more principal energy levels D) fewer principal energy levels
A
The Group 17 element with the highest electronegativity is A) fluorine C) bromine B) chlorine D) iodine
A
The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as A) first ionization energy C) conductivity B) activation energy D) electronegativity
A
The strength of an atom's attraction for the electrons in a chemical bond is the atom's A) electronegativity C) heat of reaction B) ionization energy D) heat of formation
A
Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? A) Be, Mg, Ca C) Ba, Ra, Sr B) Ca, Mg, Be D) Sr, Ra, Ba
A
Which of the following Group 2 elements has the lowest first ionization energy? A) Be B) Mg C) Ca D) Ba
A
Which sequence of elements is arranged in order of decreasing atomic radii? A) Al, Si, P C) Cl, Br, I B) Li, Na, K D) N, C, B
A
Define an ion
A charged atom
Which trend(s) can be described using the following diagram? a. ionization energy b. electronegativity c. atomic radius d. periodicity
A or b
Circle the atom in each pair that has the greater ionization energy. a)Li Be b)Na K c)Cl Si d) Ca Ba e) P Ar f) Li K
A2 B.1 C.1 D.1 E.2 F.1
Arrange the following to increasing atomic radii : Na, Mg, Al, Ar, Si, P, S, Cl
Ar, Cl, S, P, Si, Al, Mg, Na (largest)
Using the term octet, explain why electronegativity increasing from left to right on a period of the periodic table.
As you go across a period, the atom gets closer to an octet. Atoms want stability and an octet gives stability, so atoms are going to get increasingly desperate to achieve an octet as you get closer to 8 valence electrons.
Using number of protons and electrons in your argument, explain why atomic radii decreases as you go from left to right on the same period of the periodic table.
As you go across a period, the number of shells remains the same, but the number of protons increase. The increased number of protons pull the outer electrons with greater force, which causes the atom to shrink. The nucleus acts like a stronger magnet and is able to pull the outer electrons with greater force.
What causes this trend?
As you go across a period, the number of shells remains the same, but the number of protons increase. The increased number of protons pull the outer electrons with greater force, which causes the atom to shrink. The nucleus acts like a stronger magnet and is able to pull the outer electrons with greater force.
As each successive element in Group 15 of the Periodic Table is considered (going from top to bottom) in order of increasing atomic number, the atomic radius A) decreases B) increases C) remains the same
B
Which sequence correctly places the elements in order of increasing ionization energy? A) H → Li → Na → K C)O → S → Se → Te B) I → Br → Cl → F D)H → Be → Al → Ga
B
.Which trend(s) can be described using the following diagram? a. ionization energy b. electronegativity c. atomic radius d. periodicity
C
As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to A) decreasing radius and decreasing shielding effect B) decreasing radius and increasing shielding effect C) increasing radius and decreasing shielding effect D) increasing radius and increasing shielding effect
C
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? A) The relative electronegativity decreases, and the atomic radius decreases. B) The relative electronegativity decreases, and the atomic radius increases. C) The relative electronegativity increases, and the atomic radius decreases. D) The relative electronegativity increases, and the atomic radius increases.
C
Which of these elements has the least attraction for electrons in a chemical bond? A) oxygen B) fluorine C) nitrogen D) chlorine
C
B. Arrange the following groups of elements in order of decreasing (largest to smallest) electronegativity. a) C, Ge, Si b) Be, C, F C, Si, Ge F, C, Be
C, Si, Ge F, C, Be
Which is larger, Ca2+ or Ca and why?
Ca will be larger because there is a greater ratio of protons to electrons Ca2+ will be smaller because there are less electrons, so the protons can pull like a stronger magnet
What is the difference between a cation and an anion?
Cation is a positive charged ion , Anion is a negative charged ion
The ability of carbon to attract electrons is A) greater than that of nitrogen, but less than that of oxygen B) less than that of nitrogen, but greater than that of oxygen C) greater than that of nitrogen and oxygen D) less than that of nitrogen and oxygen
D
Which Group 17 element has the least attraction for electrons? A) F B) Cl C) Br D) I
D
Which element in Group 16 has the greatest tendency to gain electrons? A) Te B) Se C) S D) O
D
Which properties are most common in nonmetals? A) low ionization energy and low electronegativity B) low ionization energy and high electronegativity C) high ionization energy and low electronegativity D) high ionization energy and high electronegativity
D
Which is larger, F-1 or F and why?
F-1, there are more electrons, so the positive nucleus has a harder time pulling in all the outer electrons
Which element has the greatest electronegativity? ____________________
Fluorine
B. Arrange the following groups of elements in order of increasing (smallest to largest) ionization energy. a) Na, K, Li, Fr b) P, Ar, Cl
Fr, K, Na, Li P, Cl, Ar
. Which noble gas has the highest first ionization energy? A) radon C) neon B) krypton D) helium
Helium
Circle the atom in each pair that has the largest atomic radius. Large = further away from He a)Al B b)S O c)Br Cl d) Na Al e) O F f) Mg Ca
Its always the first one except calcium
Which of the following atoms has the largest atomic radius? A) Na B) K C) Mg D) Ca
K
Arrange the following to increasing ionization energy : N, C, B, Li, O, Ne, F
Li, B, C, N, O, F, Ne (largest)
Arrange the following to decreasing ionization energy : N, Bi, As, Sb, P
N, P, As, Sb, Bi (smallest)
What does the term "octet" mean and why do elements want an octet?
Octet means that an atom has 8 valence electrons (8 electrons in the outer shell). Atoms want to obtain an octet because it makes them stable. One exception to this would be Hydrogen and Helium, which want to obtain a duet (2 electrons) to obtain stability
Arrange the following to decreasing atomic radii: Mg, Ba, Ca, Be, Sr, Ra
Ra, Ba, Sr, Ca, Mg, Be (smallest)
Using the term shells, explain why ionization energy decreases as you go down a group on the periodic table.
Since there are more shells, the pull between the positive nucleus and the outer electrons is not at strong. Think of the solar system. The planets that are further away have less gravitational pull than the ones that are closer (Mercury has more of a pull to the sun than Neptune).
What causes this trend?
Since there are more shells, the pull between the positive nucleus and the outer electrons is not at strong. Think of the solar system. The planets that are further away have less gravitational pull than the ones that are closer (Mercury has more of a pull to the sun than Neptune).
Define electronegativity.
The ability of an atom to pull electrons to itself to form a chemical bond
What causes this trend?
The atom is getting closer to an octet. This means that atoms would prefer to gain electrons not lose them. Also, since the atom is smaller, it would be harder to pull away one of the electrons from the outer shell
Define ionization energy
The energy required to remove an electron from the outer shell (ring)
Why does atomic radius increase as you go down a group?
The increased number of shells makes the atom larger, similar to how extra layers of clothes makes a person appear larger
What causes this trend?
The larger number of shells (layers) causes the atom to become larger, similar to how putting on more layers of clothes makes you appear larger
B. Arrange the following groups of elements in order of increasing size. a) In, Tl, Ga b) Be, C, F
Tl, In, Ga F, C, Be
Does atomic radius increase or decrease as you go across a period/row on the periodic table?
decrease
What trend in electronegativity do you see as you go down a group/family on the periodic table?z
decreases
What trend in ionization energy do you see as you go down a group/family on the periodic table?
decreases
Does atomic radius increase or decrease as you go down a group/family on the periodic table?
increase
What trend in electronegativity do you see as you go across a period/row on the periodic table?
increases
What trend in ionization energy do you see as you go across a period/row on the periodic table?
increases
Arrange the following to increasing electronegativity : Te, Sn, Rb, Xe, In
nobles gases are very low electronegativity) Xe, Rb, In, Sn, Te (largest)
