unit 3 review
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Unit 3 Review. Chemistry. 1. Label the periodic groups. #1 Alkali Metals. # 2Alkaline Earth Metals. # 8 Noble Gases. # 7 Halogens. Transition Metals. 2. Circle the most EN element and square the least EN element 3. Highest IE red and lowest IE blue. Small atoms! High IE and EN. - PowerPoint PPT PresentationTRANSCRIPT
Unit 3 ReviewUnit 3 Review
ChemistryChemistry
#1 Alkali
Metals
# 2Alkaline
Earth
Metals
Transition Metals
# 7 Halogens
# 8 Noble Gases
1. Label the periodic groups1. Label the periodic groups
2. Circle the most EN element and square 2. Circle the most EN element and square the least EN elementthe least EN element
3. Highest IE red and lowest IE blue3. Highest IE red and lowest IE blue
Small atoms!
High IE and EN
LARGE atoms, low IE and EN
Lowest IE
Highest EN
5. Number the periods6. Shade period 4 blue7. The rows are periods and the columns are _______________
1
2
3
4
5
6
7
8. The periodic table is organized by_______________8. The periodic table is organized by_______________
groups
increasing atomic #
9. Use arrows to show the trend for 9. Use arrows to show the trend for increasing atomic size/radius. Circle increasing atomic size/radius. Circle
the atom with the largest size/radius.the atom with the largest size/radius.
Metals (red – for review wksht)Metals (red – for review wksht) Nonmetals (blue for review wksht)Nonmetals (blue for review wksht) Metalloids (green – for review Metalloids (green – for review
worksheet)worksheet)
11) Have 1 valence electron11) Have 1 valence electron____________________ ____________________
12) Have 8 valence electrons12) Have 8 valence electrons
____________________ ____________________
13) Have 7 valence electrons13) Have 7 valence electrons
____________________ ____________________
14) Have 2 valence electrons14) Have 2 valence electrons
Alkali metals – group 1
Noble Gases – group 18
Halogens – group 17
Alkaline Earth metals – Group 2
15) The least reactive elements15) The least reactive elements
____________________ ____________________
16) The most reactive nonmetals 16) The most reactive nonmetals (gases at room (gases at room temperature)___________________ temperature)___________________
17) The most reactive metals17) The most reactive metals
____________________ ____________________
18) Reacts explosively with oxygen 18) Reacts explosively with oxygen and waterand water____________________ ____________________
19) Used to make coins and jewelry.19) Used to make coins and jewelry.
Noble Gases
Halogens
Alkali metals
Alkali Metals
Transition Metals
20) Energy required to remove an 20) Energy required to remove an electron from an electron from an atom____________________ atom____________________
21) The ability of atom to attract 21) The ability of atom to attract electrons.electrons.
22) List 3 other elements that will have 22) List 3 other elements that will have similar chemical properties to similar chemical properties to Nitrogen and explain why.Nitrogen and explain why.
Ionization Energy
Electronegativity
Most like: Phosphorus (P)
2nd most like: Arsenic (As)
3rd most like: Antimony (Sb)
Same group –gives them same # of valence electrons and ion charge, therefore similar reactivity!
Circle the element in the pair has the Circle the element in the pair has the largerlarger ionization energy. Explain ionization energy. Explain why.why.
a. Li, Na. Li, N b. Kr, Ne b. Kr, Ne c. c. Cs, LiCs, Li
Explain the octet rule.Explain the octet rule.
Circle the element in the pair isCircle the element in the pair is more more electronegative. Explain Why?electronegative. Explain Why?
a. K, Asa. K, As b. N, Sbb. N, Sb c. Sr, Bec. Sr, Be
Closer to Fluorine!
Atoms will lose, gain, or share electrons to have 8 valence electrons in their outer energy level.
Smaller atoms – less shielding – nucleus charge is stronger and can attract the electron more easily.
Periodic law states that elements show aPeriodic law states that elements show a
a. repetition of their physical properties a. repetition of their physical properties when arranged by when arranged by increasing atomic increasing atomic radiusradius..
b. repetition of their chemical properties b. repetition of their chemical properties when arranged by when arranged by increasing atomic increasing atomic radius.radius.
c. periodic repetition of their properties c. periodic repetition of their properties when arranged by when arranged by increasing atomic increasing atomic numbernumber..
d. periodic repetition of their properties d. periodic repetition of their properties when arranged by when arranged by increasing atomic increasing atomic massmass..
Elements in the same group of the periodic Elements in the same group of the periodic table have the table have the samesame::
a.a.number of valence electronsnumber of valence electronsb.b. physical propertiesphysical propertiesc.c. number of electronsnumber of electrons
Which of the following is Which of the following is NOT NOT true of an true of an atom, other than Helium, obeying the atom, other than Helium, obeying the octet rule?octet rule?
a. obtains a full set of 8 valence electronsb. acquires the valence electrons of a
noble gasc. possess 8 electrons in totald. has a s2p6 valence configuration
Moving down the periodic table, which two Moving down the periodic table, which two atomic properties follow the same atomic properties follow the same trend?trend?
a. atomic radius, ionization energya. atomic radius, ionization energyb. atomic radius, electronegativityb. atomic radius, electronegativityc. ionization energy, electronegativityd. none of the aboved. none of the above
Which will form a larger ionic radii than its’ Which will form a larger ionic radii than its’ parent atom? parent atom? a. cationa. cation (+ ion) (+ ion) b. anion (- ion)
Explain your choice!Explain your choice! Extra electrons cause repulsion and cloud spreads out – ion gets bigger!
23) How many electrons does an atom 23) How many electrons does an atom of Oxygen have? _____of Oxygen have? _____
How many valence electrons?________How many valence electrons?________
How many electrons does 0How many electrons does 0-2-2 have? have? __________
24) Fluorine has a higher ionization 24) Fluorine has a higher ionization energy than oxygen because fluorine energy than oxygen because fluorine has a larger ____________ charge (why has a larger ____________ charge (why fluorine holds on to its electrons so fluorine holds on to its electrons so well)well)
8 total
10 total, 8 valence
NUCLEAR/positive
6
1s1s22 2s 2s22 2p 2p66 3s 3s22 3p 3p66 4s 4s22
25) Which element is this for? 25) Which element is this for? ____________________-____________________-
26) In which period is this element 26) In which period is this element found in?______found in?______ In which group #? In which group #? ______________
27) How many electrons are in 27) How many electrons are in this this element’s 3rd energy level? _____element’s 3rd energy level? _____
28) Re-write the electron configuration 28) Re-write the electron configuration of this element if it became an ion of this element if it became an ion with a with a +2+2 charge charge
Calcium
4 2
8
1s1s22 2s 2s22 2p 2p66 3s 3s22 3p 3p66
It loses the 2 electrons in 4s
29) What is an orbital? A ____________ 29) What is an orbital? A ____________ shaped region of an atom where an shaped region of an atom where an ____________ is most likely to be ____________ is most likely to be found.found.
30) How many 30) How many orbitals (circles)orbitals (circles) are in are in each sublevel? a. S = ___ b. P = each sublevel? a. S = ___ b. P = ___ ___
c. d = ___ d. F = ____c. d = ___ d. F = ____
31) How many electrons can fit into 1 31) How many electrons can fit into 1 orbital? _____orbital? _____
Cloud Shaped
Electron
1 3
5 7
2 electrons
32) Is the following electron sketch 32) Is the following electron sketch correct? correct? ExplainExplain
3s 3p 4s 3d
It is not correct, the 3d orbitals should have one in each orbital and then it should double up!
33) Label the following 33) Label the following blocksblocks
34) Identify the blocks where these 34) Identify the blocks where these groups are found –groups are found –
a. Halogens = ____ blocka. Halogens = ____ block
b. Alkaline Earth Metals = _____ blockb. Alkaline Earth Metals = _____ block
c. Alkali Metals = ______ blockc. Alkali Metals = ______ block
d. Rare Earth Metals = ______ blockd. Rare Earth Metals = ______ block
e. The Noble Gases = _____ blocke. The Noble Gases = _____ block
f. The Transition Metals = _______ f. The Transition Metals = _______ blockblock
p
s
s
f
p
d
35) 35) Identify Identify
the the spectruspectru
mm
A: Hydrogen & Helium B: Helium, Barium, Sodium
C: Barium, Calcium, Hydrogen, Helium
Photons and the Electromagnetic Photons and the Electromagnetic
SpectrumSpectrum
36) An electron that is closest to the 36) An electron that is closest to the nucleus possible (at the lowest nucleus possible (at the lowest energy level possible) is said to be in energy level possible) is said to be in its ___________ _________________.its ___________ _________________.
37) When an electron jumps up to a 37) When an electron jumps up to a higher energy level and then falls higher energy level and then falls back to its ground state a ___________ back to its ground state a ___________ is released. is released.
Ground State
Photon
Photons and the Electromagnetic Photons and the Electromagnetic
SpectrumSpectrum 38) The amount of energy released by an 38) The amount of energy released by an
electron jumping from the 4th energy level electron jumping from the 4th energy level back to its ground state at the 3rd energy back to its ground state at the 3rd energy level will always release a photon with level will always release a photon with a___________________________ (different-a___________________________ (different-variable/variable/specific-quantizedspecific-quantized) amount of ) amount of energy.energy.
39) The color spectra (types of colors 39) The color spectra (types of colors produced) of a star can be used to identify produced) of a star can be used to identify the types of ______________ present in the the types of ______________ present in the star.star.
Elements