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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.

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1 label the periodic groups
1. Label the periodic groups

#1 Alkali


# 2Alkaline



# 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
2. Circle the most EN element and square the least EN element3. Highest IE red and lowest IE blue

Small atoms!

High IE and EN

Highest EN

Lowest IE

LARGE atoms, low IE and EN

5 number the periods 6 shade period 4 blue 7 the rows are periods and the columns are
5. Number the periods6. Shade period 4 blue7. The rows are periods and the columns are _______________









increasing atomic #

8. The periodic table is organized by_______________

9. Use arrows to show the trend for increasing atomic size/radius. Circle the atom with the largest size/radius.
Metals (red – for review wksht)

Nonmetals (blue for review wksht)

Metalloids (green – for review worksheet)


Alkali metals – group 1

11) Have 1 valence electron ____________________

12) Have 8 valence electrons


13) Have 7 valence electrons


14) Have 2 valence electrons

Noble Gases – group 18

Halogens – group 17

Alkaline Earth metals – Group 2


Noble Gases

15) The least reactive elements


16) The most reactive nonmetals (gases at room temperature)___________________

17) The most reactive metals


18) Reacts explosively with oxygen and water ____________________

19) Used to make coins and jewelry.


Alkali metals

Alkali Metals

Transition Metals


Ionization Energy

20) Energy required to remove an electron from an atom____________________

21) The ability of atom to attract electrons.

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


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 larger ionization energy. Explain why.

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

Explain the octet rule.

Circle the element in the pair is more electronegative. Explain Why?

a. K, As b. N, Sb c. 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 a

a. repetition of their physical properties when arranged by increasing atomic radius.

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

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

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


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

  • number of valence electrons
  • physical properties
  • number of electrons
  • Which of the following is NOT true of an atom, other than Helium, obeying the octet rule?
  • a. obtains a full set of 8 valence electrons
  • b. acquires the valence electrons of a noble gas
  • c.possess 8 electrons in total
  • d. has a s2p6 valence configuration
Moving down the periodic table, which two atomic properties follow the same trend?

a. atomic radius, ionization energy

b. atomic radius, electronegativity

c. ionization energy, electronegativity

d. none of the above

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

a. cation (+ ion) b. anion (- ion)

Explain your choice!

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


8 total

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

How many valence electrons?________

How many electrons does 0-2 have? _____

24) Fluorine has a higher ionization energy than oxygen because fluorine has a larger ____________ charge (why fluorine holds on to its electrons so well)


10 total, 8 valence


1s 2 2s 2 2p 6 3s 2 3p 6 4s 2
1s2 2s2 2p6 3s2 3p6 4s2

25) Which element is this for? ____________________-

26) In which period is this element found in?______ In which group #? _______

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

28) Re-write the electron configuration of this element if it became an ion with a +2 charge





1s2 2s2 2p6 3s2 3p6

It loses the 2 electrons in 4s


Cloud Shaped


29) What is an orbital? A ____________ shaped region of an atom where an ____________ is most likely to be found.

30) How many orbitals (circles) are in each sublevel? a. S = ___ b. P = ___

c. d = ___ d. F = ____

31) How many electrons can fit into 1 orbital? _____





2 electrons

32) Is the following electron sketch correct? Explain

3s 3p 4s 3d

It is not correct, the 3d orbitals should have one in each orbital and then it should double up!



34) Identify the blocks where these groups are found –

a. Halogens = ____ block

b. Alkaline Earth Metals = _____ block

c. Alkali Metals = ______ block

d. Rare Earth Metals = ______ block

e. The Noble Gases = _____ block

f. The Transition Metals = _______ block






35 identify the spectrum
35) Identify the spectrum

A: Hydrogen & Helium

B: Helium, Barium, Sodium

C: Barium, Calcium, Hydrogen, Helium

photons and the electromagnetic spectrum
Photons and the Electromagnetic Spectrum

36) An electron that is closest to the nucleus possible (at the lowest energy level possible) is said to be in its ___________ _________________.

37) When an electron jumps up to a higher energy level and then falls back to its ground state a ___________ is released.

Ground State


photons and the electromagnetic spectrum1
Photons and the Electromagnetic Spectrum

38) The amount of energy released by an electron jumping from the 4th energy level back to its ground state at the 3rd energy level will always release a photon with a___________________________ (different-variable/specific-quantized) amount of energy.

39) The color spectra (types of colors produced) of a star can be used to identify the types of ______________ present in the star.