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