Unit 3 ReviewUnit 3 Review

Honors ChemistryHonors Chemistry

1-Alkali

Metals

2-Alkaline

Earth

Metals

3-12 Transition Metals

17-Halogens

18- Noble Gases

Small atoms!

High IE and EN

High IE and EN

Highest IE

Lowest IE

Highest EN

Organized by increasing atomic Organized by increasing atomic numbernumber

1

2

3

4

5

6

7

Atomic Radius TrendsAtomic Radius Trends

Bigger down-

More energy levels!

Smaller across period – higher nuclear charge

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

____________________ ____________________

12) Have 7 valence electrons12) Have 7 valence electrons

____________________ ____________________ 13) Have 2 valence electrons13) Have 2 valence electrons

Alkali metals – group 1

Noble Gases – group 18

Halogens – group 17

Alkaline Earth metals – Group 2

14) The least reactive elements14) The least reactive elements

____________________ ____________________ 15) The most reactive nonmetals 15) The most reactive nonmetals

(gases at room temperature)(gases at room temperature)

____________________ ____________________ 16) The most reactive metals16) The most reactive metals

____________________ ____________________ 17) Reacts readily with oxygen and 17) Reacts readily with oxygen and

waterwater

____________________ ____________________ 18) Used to make coins and jewelry.18) Used to make coins and jewelry.

Noble Gases

Halogens

Alkali metals

Alkali Metals

Transition Metals

19) Energy required to remove an 19) Energy required to remove an electron from an atomelectron from an atom

____________________ ____________________ 20) The ability of atom to attract 20) The ability of atom to attract

electrons.electrons.

21) List 3 other elements that will 21) List 3 other elements that will have similar chemical properties to have similar chemical properties to Nitrogen and explain why.Nitrogen and explain why.

Ionization Energy

Electronegativity

Phosphorus, Arsenic and Antimony

Same group –gives them same # of valence electrons and ion charge, therefore similar reactivity!

22. Circle the element in the pair 22. Circle the element in the pair has the has the largerlarger ionization energy. ionization energy. Explain why.Explain why.

a. Li, Na. Li, N b. Kr, Ne b. Kr, Ne c. c. Cs, LiCs, Li

23. Explain the octet rule.23. Explain the octet rule.

24. Circle the element in the pair is24. Circle the element in the pair is moremore electronegative. Explain Why? electronegative. Explain Why?

a. K, Asa. K, As b. N, Sbb. N, Sb c. Sr, Bec. Sr, Be

Smaller atoms – have less shielding – higher nuclear charge to hold on to its valence electrons!

Atoms will lose or gain 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.

25. Periodic law states that elements show a25. Periodic law states that elements show a a. repetition of their physical properties when arranged by a. repetition of their physical properties when arranged by

increasing atomic radiusincreasing atomic radius.. b. repetition of their chemical properties when arranged by b. repetition of their chemical properties when arranged by

increasing atomic radius.increasing atomic radius. c. periodic repetition of their properties when arranged by c. periodic repetition of their properties when arranged by

increasing atomic numberincreasing atomic number.. d. periodic repetition of their properties when arranged by d. periodic repetition of their properties when arranged by

increasing atomic massincreasing atomic mass..

26. Elements in the same group of the periodic table have the 26. Elements in the same group of the periodic table have the same:same:

a. number of valence electronsa. number of valence electrons b. physical propertiesb. physical propertiesc. number of electronsc. number of electrons

27. Which of the following is 27. Which of the following is NOT NOT true of an atom, other than true of an atom, other than Helium, obeying the octet rule?Helium, obeying the octet rule?

a. obtains a full set of 8 valence electronsa. obtains a full set of 8 valence electrons b. acquires the valence electrons of a noble gasb. acquires the valence electrons of a noble gas c. possess 8 electrons in totalc. possess 8 electrons in total d. has a sd. has a s22pp66 valence configuration valence configuration

28. Moving down the periodic table, which 28. Moving down the periodic table, which two atomic properties follow the same two atomic properties follow the same trend?trend?

a. atomic radius, ionization energya. atomic radius, ionization energy b. atomic radius, electronegativityb. atomic radius, electronegativity c. ionization energy, c. ionization energy,

electronegativityelectronegativity d. none of the aboved. none of the above

29.29. Which will form a larger ionic radii than Which will form a larger ionic radii than its’ parent atom? its’ parent atom?

a. cationa. cation (+ ion) (+ ion) b. anion (- ion)b. anion (- ion) Explain your choice!Explain your choice!

Extra electrons cause repulsion and cloud spreads out – ion gets bigger!

30) How many electrons does an atom 30) How many electrons does an atom of Oxygen have? _____of Oxygen have? _____

How many electrons does 0How many electrons does 0-2-2 have? have? __________

31) Fluorine has a higher ionization 31) 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, 6 valence electrons 10 total,

8 valence

NUCLEAR

1s1s22 2s 2s22 2p 2p66 3s 3s22 3p 3p66 4s 4s22 3d 3d66

32) Which element is this for? 32) Which element is this for? ____________________-____________________-

33) In which period is this element 33) In which period is this element found in?______found in?______ In which group #? In which group #? ______________

34) How many electrons are in 34) How many electrons are in this this element’s 3rd energy level? _____element’s 3rd energy level? _____

35) Re-write the electron configuration 35) 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

Fe - Iron

4 8

14

1s1s22 2s 2s22 2p 2p66 3s 3s22 3p 3p66 3d 3d66 It loses the 2 electrons in 4s

d-orbitals do not change!

36) What is an orbital? A ____________ 36) 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.

37) How many 37) How many orbitalsorbitals are in each are in each sublevel? a. S = ___ b. P = ___ sublevel? a. S = ___ b. P = ___ c. d = ___ d. F = ____c. d = ___ d. F = ____

38) How many electrons can fit into 1 38) How many electrons can fit into 1 orbital? _____orbital? _____

Cloud Shaped

Electron

1 3 5

7

2 electrons

39) What do the quantum numbers tell 39) What do the quantum numbers tell us about an atomic orbital?us about an atomic orbital?

•The probable location of an electron

•The main energy level it is on.

•The shape of the orbital (s, p, d or f) it is in.

•The orientation of that orbital around the nucleus

•The spin direction of the electron

40) Is the following orbital notation for 40) Is the following orbital notation for the 3rd and 4th energy levels of the the 3rd and 4th energy levels of the element in #32 above correct? element in #32 above 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!

#40#40

41) Identify the blocks where these 41) Identify the blocks where these groups are found –groups are found –

a. Halogens = ____ blocka. Halogens = ____ block b. Alkaline Earth Metals = _____ b. Alkaline Earth Metals = _____

blockblock c. Alkali Metals = ______ blockc. Alkali Metals = ______ block d. Rare Earth Metals = ______ d. Rare Earth Metals = ______

blockblock e. The Noble Gases = _____ blocke. The Noble Gases = _____ block f. The Transition Metals = _______ f. The Transition Metals = _______

blockblock

p

s

s

f

p

d

Photons and the Electromagnetic Photons and the Electromagnetic

SpectrumSpectrum 41) An electron that is closest to the 41) 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 ___________ _________________.

42) When an electron jumps up to a 42) 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 43) The amount of energy released by an 43) 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.

44) The color spectra (types of colors 44) 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