The periodic table test
Groups
(Think families) Vertical columns, up/down the periodic table Numbers on top of columns designate group number 1,2,13,14 etc
What is the normal boiling point of argon? 202 degrees Celsius 87 degrees Celsius -334 degrees Celsius -186 degrees Celsius
-186 degrees Celsius
Element X,Y, and Z are located in the same group on the periodic table and listed in order of increasing atomic number. The melting point of C is 100K and the melting point of Z is 200K. Which of the following is most likely the melting point of Y? 90K 150K 210K 220K
150K bc it is in between 100 and 200
WhT happens when Sr forms Sr^2+ ion?
2 electrons lost and radius decreases
Electron configuration of Na^+1 ion Number of electrons lost or gained
2-8 1 lost
Electron configuration of Na atom
2-8-1
Electron configuration of Cl atom
2-8-7
What is the electron configuration of S^2-
2-8-8
Electron configuration of Cl^1- ion Number of electrons lost or gained
2-8-8 1 gained
An atom of an element has 18 electrons, what period does this element belong in?
3
Which electron dot represents an alkali metal? 1) x with 8 dots 2) x with 2 dots 3) x with 1 dot 4) x with 5 dots
3) x with 1 dot
Which value would most likely represent the ionization energy of a metal? 393 kj/mole 1000 kj/mole 1251 kj/mole 1351 kj/mole
393 kj/mole
An ion is
A charged particle, NOT NEUTRAL
Ionization energy high=
A lot of energy to remove electrons=NONMETAL
What are the remaining elements in period 3? Na and Mg
Al, Si, P, S, Cl, Ar
An element with 2 valence electrons in the 4th principal energy level is classified as an Alkali metal Alkaline Earth metal Metalloid
Alkaline earth metal
Allotropes of nonmetals
An allotrope is a different form (molecular arrangement) of the same element
Electronegativity
An atoms ability to attract electrons in a chemical bond
Where does the charge (+/-) come from?
An unequal number of protons and electrons
Cl^1- has the same electron configuration as what group 18 element?
Ar
The elements on the periodic table are arranged according to increasing
Atomic number
Which atom will have the least attraction for electrons in a chemical bond? Be Mg Ca Ba
Ba
Which atom can lose an electron most readily? Be Ca Ba
Ba bc lowest ionization energy
Which is the most metallic group 15 element? N As Bi
Bi
Which of the following has a boiling point closest to the temperature at STP? F Cl Br
Br
Give the symbol of one element that is a liquid at room temperature
Br Hg
Diatomic are
Br I N Cl H O F
If nonmetal, how do you set up the Lewis dot structures of ions
Brackets, charge, 8 dots
If metal, how do you set up the Lewis dot structures of ions
Brackets, charge, no dots
Which of e following is an electron configuration of a period 4 element? A. 2-1 B. 2-8 C. 2-8-18-2 D. 2-8-4
C. 2-8-18-2
Which set has valence electrons in the same energy shell? A. Na, K, Rb B. Ca, Mn, I C. Mg, P, Cl
C. Mg, P, Cl
What are the remaining elements in group 2?
Ca, Sr, Ba, and Ra
Chemical properties _______ across a ______.
Change Period
Which atom will have the most attraction for electrons in a chemical bond? Cl P Al Mg
Cl
Which of the following has an atomic radius that is smaller that it's ionic radius? Na or Cl
Cl
Which compound forms a colored solution? NaCl Al(NO3)3 CrPO4
CrPO4
Metallic character increases or decreases as you go from left to right on the P.T.?
Decreases
Allotropes of the same element have
Difference chemical properties and different physical properties
Metalloids
Elements that touch the stair case B, Si, Ge, As, Sb, and Te
Metals
Elements to the left of the staircase
Nonmetals
Elements to the right of the staircase H is a nonmetal
Which atom requires the most amount of energy to remove the outermost electron? Li N F
F
Which has a larger radius Be^2+ or F^-? Explain your answer because on atomic structure.
F^- Because 2-8
Notes on group numbers
For groups 13-18, subtract 10 to get the number of valence electrons. Examples: An element in group 18 has 8 valence electrons An element in group 15 has 5 valence electrons An element group 2 has 2 valence electrons (not in groups 13-18)
Nonmetals typically gain electrons to...
Form negative ions
Group 17 on the periodic table is
Halogens
Which noble gas does Li* have the same electron configuration as?
Helium (2-1)
Periods
Horizontal rows, across the periodic table. Numbers to the left of the periodic table designate the period 1,2,3,4 etc
Groups of the periodic table: Alkali metals Characteristics (6) (Li, Na, K, Rb, Cs, Fr)
If X represents any element in group 1, draw the electron dot structure for X: which is X and one dot. Very reactive due to 1 valence electron, very easy to lose an electron Further down=more reactive Group 1 metals are so reactive they are only found in compounds (I.e. NaCl) in nature General formula of group 1 oxides: X2O General formula of Group 1 chlorides: XCl
Groups of the periodic table Group 16: Halogens characteristics (5)
If X represents any element in group 17, the electron dot structure is X with 7 dots Very reactive nonmetals due to electron configuration only need 1 electron for full valence shell F is the most reactive nonmetal on the periodic table. So reactive it can combine with Group 18 Group 16 occur as compounds in nature (ex NaF) or as Diatomic- F2, Cl2, Br2, I2 At room temperature, only group on the periodic table with elements as a solid,liquid, and gas
Groups of the periodic table Group 17: Noble gases characteristics (3)
If X represents any element in group 18, the electron dot structure is X either with 2 dots or with 8 dots Group also includes He, 2 valence electrons Very unreactive (stable) due to full valence shell (mostly have only oxygen state of 0) Occur naturally as monatomic gases
Groups of the periodic table: Alkaline Earth Metals Characteristics (5) Be, Mg, Ca, Sr, Ba, Ra
If X represents any element in group 2, draw the electron dot structure for X: which is X with two dots on the same side. Also very reactive, but not as reactive as group 1 metals Also only found in compounds (I.e. CaCl2) in nature General formula of Group 2 oxides: XO General formula of Group 2 chlorides: XCl2
When a trend increases across a period, what is the explanation? (Ionization/electronegativity)
Increased nuclear charge
When going down a group and the trend decreases what is the explanation for it (ionization/electronegativity)
Increased number of energy levels and/or increased shielding
The radius of a nonmetal ion compared to a nonmetal atom is...
Larger
Ionization energy low=
Little energy to remove electrons=METAL
When an Al atom becomes an Al+3 ion elements are lost/gained and radius increases/ decreases.
Lost Decreases
Metal properties (8)
Malleable Ductile (make into wires) Have luster (shiny) Good conductors of heat and electricity Solids at room temperature: one exception is Hg(mercury) because it is a liquid at room temperature Low ionization energy Low electronegativity Metals lose electrons to form positive ions
Of the following, which is the most metallic element: Mn, Ge, Se, & Br
Mn (manganese)
Which is the most nonmetallic group 15 element? N As Bi
N
Which of the following have the most similar chemical properties: B, C, N, O, P A) explain answer based on atomic structure B) explain answer based on the periodic table
N and P A)they have the same number of valence electrons B) they are both in group 15
Which has a greater radius Na or Na+1, explain your answer based on atomic structure?
Na bc Na+1 loses an energy level
Nonmetals gain electrons to form what?(atomic radius compared to ionic radius)
Negative ions
Na^+1 has the same electron configuration as what group 18 element?
Neon
When Ca loses 2 electrons and becomes Ca^2+, what happens to the number of protons in the nucleus?
No change
Group 15 & 16 on the periodic table is
No name
An element has 7 valence electrons and 3 occupied principal energy levels. Is this a metal, nonmetal, or metalloids?
Nonmetal
Ide endings are given to
Nonmetal ions
Period # indicates the
Number of energy levels or energy level where valence electrons are found
What are the allotropic forms of oxygen, carbon, and sulfur?
Oxygen: O2/O3 (ozone) Carbon: diamond/graphite/coal/fullerene Sulfur. Yellow/res
An element has 5 valence electrons in the 3rd principal energy level, what element is this?
P
Give the period number and group number of one diatomic element
Period 2, group 15-> N
Metals lose electrons to form what? (Atomic radius compared to ionic radius)
Positive ions
Metals lose electrons to form...
Positive ions
Groups of the periodic table Group 15&16 characteristics (3)
Properties change from nonmetallic to metallic down the group (cross the staircase) Properties change form metallic to nonmetallic across the period (cross the stair case) Metalloids have properties of metals and nonmetals
Periodic law
Properties of the elements are functions of their atomic number. Because of periodic law, the properties of new elements, not yet discovered, could be predicted.
Elements in the same group have
Similar chemical properties because they have the same number of valence electrons
The radius of a metal ion compared to a metal atom is...
Smaller
Nonmetal properties (7)
Solids are brittle (sulfur and carbon) Lack luster (dull) Poor conductors of heat and electricity Usually solid/gas at room temperature: one exception is Bromine (Br) is a liquid at room temperature High ionization energy High electronegativity Nonmetals gain electrons to form negative ions
Electronegativity HIGH=
Strong attraction electrons=NONMETAL
Booming point and melting point can be found in
Table S
Atomic radius
The disgrace form the nucleus to the valence electrons
First ionization energy
The energy required to remove an electron from an atom
The ion a metal CAN become is...
The oxidation state found in the upper right corner of element symbol
Groups 3-12 are
Transition metal elements and will be dealt with separately
Groups of the periodic table: transition metals Characteristics 3-12
Transition metals with multiple positive oxidation states Use electrons from more than one energy level when bonding Compounds form colored solutions, CuSO4(aq)=blue solution
Electronegativity low=
Weak attraction for electrons= METAL
Group 1 on the periodic Table is
alkali metals
Group 2 on the periodic table is
alkaline earth metals
Group 18 on the periodic table is
noble gases
Group 3-12 on the periodic table is
transition metals
