Chapter 6 Periodic Table

A
In which set of elements would all members be expected to have very similar chemical properties?
a) O, S, Se
b) S, Se, Si
c) Ne, Na, Mg
d) N, O, F
e) Na, Mg, K
C
Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si, and Ar?
a) Ar > Si > P > Na > Mg
b) Si > P > Ar > Na > Mg
c) Na > Mg > Si > P > Ar
d) Mg > Na > P > Si > Ar
e) Ar > P > Si > Mg > Na
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B
Which elements would be expected to have chemical and physical properties closes to those of fluorine?
a) Fe
b) Cl
c) O
d) S
e) Ne
B
Which one of the following is NOT true about the alkali metals?
a) They are very reactive elements.
b) They all have 2 electrons in their valence shells.
c) They have the lowest first ionization energies of the elements.
d) They are low density solids at room temperature.
e) They all readily form ions with a +1 charge.
C
The alkali metal that is naturally radioactive is ________________.
a) lithium
b) cesium
c) francium
d) rubidium
e) sodium
A
Atomic radius generally increases as we move _______________.
a) down a group and from right to left across a period.
b) down a group and from left to right across a period.
c) down a group, the period position has no effect,
d) up a group and from left to right across a period.
e) up a group and from right to left across a period.
D
Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is _______________.
a) Na
b) K
c) Ra
d) Sr
e) Be
C
Of the following elements, which has the largest first ionization energy?
a) B
b) Si
c) N
d) C
e) P
A
The most common sulfur ion has a charge of _________________.
a) 1 minus
b) 2 minus
c) 4 plus
d) 6 plus
e) sulfur does not form ions
A
Of the choices below, which gives the order for first ionization energy?
a) Ar > Cl > S > Si > Al
b) S > SI > Cl > Al > Ar
c) Cl > S > Al > Ar > Si
d) Al > Si > S > Cl > Ar
e) Cl > S > Al > Si > Ar
A
Alkali metals tend to be more reactive than alkaline earth metals because ____________.
a) alkali metals have lower ionization energies
b) alkali metals have lower densities
c) alkali metals have lower melting points
d) alkali metals have greater electron affinities
e) alkali metals are not more reactive than alkaline earth metals
D
Of the halogens, which are gases at room temperature and atmospheric pressure?
a) flourine, chlorine, and bromine
b) flourine, bromine, iodine
c) flourine, chlorine, iodine
d) flourine and chlorine
e) flourine, chlorine, bromine, and iodine
D
This element is more reactive than lithium and magnesium but less reactive than potassium. This element is _______.
a) Rb
b) Be
c) Ca
d) Na
e)Fr
D
Of the following elements, __________ has the most negative electron affinity.
a) Na
b) N
c) Be
d) F
e) Li
B
Which one of the following is a metalloid?
a) Br
b) Ge
c) C
d) Pb
e) S
A
The first ionization energies of the elements _________ as you go from left to right across a period of the periodic table, and _____________ as you go from the bottom to the top of a group in the table.
a) increase, increase
b) increase, decrease
c) decrease, increase
d) decrease, decrease
e) are completely unpredictable
D
Metals can be _______ at room temperature.
a) solid, liquid, or gas
b) solid only
c) liquid or gas
d) solid or liquid
e) liquid only
A
In general, as you go across a period in the periodic table from left to right:
1) the atomic radius __________
2) the electron affinity becomes ________ negative; and
3) the first ionization energy__________
a) decreases, increasingly, increases
b) increases, increasingly, increases
c) decreases, increasingly, increases
d) increases, increasingly, decreases
e) decreases, decreasingly, increases
B
Consider the following properties of an element:
i) It is solid at room temperature
ii) it easily forms an oxide when exposed to air
iii) when it reacts with water, hydrogen gas evolves.
iv) it must be stored submerged in oil.
Why element fits the above description best?
a) sulfur
b) sodium
c) mercury
d) magnesium
e) copper
B
Which nonmetal exists at a diatomic solid?
a) antimony
b) iodine
c) phosphorus
d) boron
e) bromine
A
Of the following elements below, ___________ is the most metallic.
a) K
b) Na
c) Al
d) Ar
e) Mg
D
Which ion below has the largest radius?
a) F minus
b) Cl minus
c) K plus
d) Br minus
e) Na plus
E
The ____________ have the most negative electron affinities.
a) alkaline earth metals
b) chalcogens
c) transition metals
d) alkali metals
e) halogens
C
Which of the following traits characterizes the alkali metals?
a) existence as diatomic molecules
b) the smallest atomic radius in a period
c) the lowest first ionization energies in a period
d) very high melting point
e) formation of dianions
C
Elements in the modern version of the periodic table are arranged in order of increasing
a) average atomic mass
b) atomic mass
c) atomic number
d) number of isotopes
e) oxidation number
B
Nonmetals can be _________ at room temperature.
a) liquid or gas
b) solid, liquid, or gas
c) solid or liquid
d) liquid only
e) solid only
E
Most of the elements on the periodic table are __________.
a) nonmetals
b) metalloids
c) gases
d) liquids
e) metals
D
Which one of the following atoms has the largest radius?
a) Ne
b) Cl
c) F
d) S
e) O
C
All the elements in group VIIIA are gases at room temperature. Of all the groups in the periodic table, only group ______ contains examples of elements that are gas, liquid, and solid at room temperature.
a) IIA
b) VIA
c) VIIA
d) VA
e) IA
B
____________ is a unique element and does not truly belong to any family.
a) Helium
b) Hydrogen
c) Uranium
d) Radium
e) Nitrogen
arranged atoms by increasing atomic number
What was Mosley’s achievement(s)?
arranged atoms by increasing atomic mass
What was Mendeleyev’s achievement(s)?
law of octaves
What was Newland’s achievement(s)?
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