Chapter 4 and 5

Test 1Workshop 1Test 2Workshop 2Test 3 Workshop 3Test 4 Workshop 4Middle Exam

T Chemistry Test #1

Electron Configuration and Periodic PropertiesSeptember 23, 2013 Name_________________________10º ___30pts. Student ScoreDo not scratch, or erase. Check your spelling. Use pen only.Answer the following questions. Be clear neat. One point each

1. Match the outermost electron configuration with the corresponding property. You may use them Several times or none.

4 P6 Higher electronegativity ______

2 P3 Higher reactivity ______

4 S1 Lower atomic radius ______

5 F6 Lower ionization electrons ______

4 P4 Eight valence electrons ______ It forms ions 4- ______

2. The properties of the element 120 would be: (write high or low where necessary)Ionization energy _____ atomic radius ______ reactivity ______ electronegativity _______ electronAffinity ______ type of ion __________ metallic character _________ # valence electrons _______

3. Three isoelectronic ions are: _____________________________________4. Predict the formula that better represents the compound when indium combines with

iodine by usingThe following information: GaP, GaF3, Al2O3 _________________________

5. The successive ionization energies (in kJ/mol) for an unknown element are:IE1: 1314 IE2: 3388 IE:5300 IE4: 7469 IE5: 10990To which group number in the periodic table the unknown element most likely belong? ______________

6. The noble gas configuration of TI 3+¿ ¿ is ________________________7. Write the equation for the electron affinity of Cl. The electron affinity is -36107 kJ/mol,

____________________________________

8. Arrange them in decreasing order of their size: K+¿ ¿, Ca2+¿ ¿, Ar, Cl−¿¿, S2−¿¿

__________________________9. Would you expect the electron affinities for the three isotopes of hydrogen, hydrogen,

deuterium andTritium to be the same of different? _________________________

10. Along with the increased distance of the outer electron from the nucleus, the __________________ of the

Inner electrons causes ionization energy to decrease going down a column of the periodic table .

11. The atomic radius of F, Cl, and I are 64,89 and 138 pm respectively. From this information (and not yourBook) estimate a reasonable atomic radius of Br from thelist: S3, 198,26,162,114 ____________

12. Rank each of the following in order of INCREASING electronegativity : V,Y,O ____________13. Rank each of the following in order of DECREASING ionization energy: Cl,Cu,Au

_________________14. Rank each of the following in order of DECREASING atomic radius : Os, Ni, Fe

________________15. Rank each of the following in order of INCREASING metallic character: Mn, Nb, Ir, Hf

________________16. Which property is illustrated in the graph across a period?

_____________________________

17. I am one of the elements. I have the highest ionization energy in my group. I increase in size when I

Become an ion and it is higher than the element at my left. The elemente at my left has a smallerElectron affinity but the element at my right has a more positive electron affinity and I do not why. I Have no d electron and I am necessary for the existence of living matter. Who am I? _______ (symbol)Support your answer. (2 points)

Second Quarter: Chemistry Workshop #1

10 grades

Electron Configuration and Periodic Properties

Date ________________ Name ________________

Answer the following questions. Be clear and neat

1. I am one of the elements. I have a high electron affinity (highly negative value), and my atomic number is X. The element with atomic number X-1 has lowest ionization energy and a lower electron affinity (less negative value).The element with atomic number X+1 has higher ionization energy and basically no electron affinity (positive value). I am toxic and reactive in my elemental state, but I am very commonly found in my nontoxic ionic state. Within my group, I have the second highest ionization energy. Who am I? Support your answer.

2. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.

3. Which species of each pair has the largest radius?

K+ or Cl P3 or N3

4. Order the following groups from largest to smallest radiia) Ar, Cl, K+, S2- b) Na, Mg, Ar, P

5. For each of the following pairs, which of the two species is smaller?a) K+ or Li+ b) P3- or N3-

6. Pick a noble gas, write its shorthand e- configuration and determine its number of electrons. Then find the halogens, alkali metal and alkaline earth metal with the

same number of electrons. Write these as their most stable ion. They will constitute an isoelectronic series

Noble Gas Alkali metal Alkaline earth metal

Halogen

Species symbolElectron configuration

Z# of electronsOrder them by increasing atomic or ionic radius.

7.1. Which is the largest atom in Group IV?

7.2. Which is the smallest atom in Group VII?

7.3. Which is the smallest atom in period 5?

8. Which species of each pair has the higher Ionization energy?

A. Mg or Mg2+

B. O or O2-

C. K+ or Cl-

9. Which of the following has the largest IE2?

A. KB. CaC. ScD. Fe

10. Shown below are the Ionization energies for three elements in the third period. Label each box with the correct element

IE1 IE2 IE3 IE4496 4560 6912 9543737 1451 7733 10,540578 1816 2744 11,577

11. Choose the orbital in which an electron would experience the highest Z, effective nuclear charge (least shielded), an highest IE1

A. Na (3s)B. Mg (3s)C. Al (3p)D. P (3p)E. S (3p)

12. Match the following electron configuration with the appropriate Ionization energies (IE1)

A. 1s22s2 2p63s24s23d10 4p65s1 hjk1356 kj/molB. 1s2 2s2 2p6 3s2 3p6 4s2mkl595 kj/molC. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 mkl409 kj/mol

13. Why do you think sodium has more negative electron affinity value than magnesium?

14. Nitrogen has a positive value for electron affinity, yet oxygen has a negative value. Explain this using an orbital diagram

15. Rank the following by increasing electronegativity: N, P, O

16. Choose from the following atoms to answer the next 4 questions

(A) Fluorine

(B) Oxygen

(C) Lithium

(D) Sodium

(E) Potassium

Which element is the least electronegative?

Which element has the lowest ionization energy?

Which element has the smallest ion?

Which atom has the smallest atomic radius?

17. The following is a list of the charge found on the ions of a series of elements:

Y+ W2* Z2+ V3+ X+

State which elements are most likely to be metals

18. Given the valence electron configuration of elements a, b, c and d :

A. 4s1 B. 5s1 C. 5s2 D.5sp3

Which elements have the lowest first ionization energy? _______________________

19. Which of these elements would have the lowest first ionization energy? Has one valence electron and forms X+?

Element A Element B Element C Element D

20. The chemical formulas for the oxides of potassium, calcium, gallium and germanium are, respectively, K2O, C2O, Ga2O2 and GeO2. Refer to the periodic table and predict the chemical formula for each of the following compounds: Explain

(a) Rubidium oxide

(b) Strontium oxide

(c) Indium oxide

(d) Lead oxide

21. Predict which of the following metals has chemical properties most similar to Zinc : Fe, Cu or Cd.

22.Write the noble gas electron configuration for each of the following

(a)Cd2+ (b) P3-

Ionic Bonds and Ionic Compound / Metallic Bonding

Short Answers (2 points each one)

A. Cristal lattice of metals is formed by

B. Metals are good conductors of heat. Why?

C. Write the fallowing substances in increasing order of the properties indicated:a) Cristal lattice of CaO, Sr3P2, MgO b)Melting Point of LiCl, Li2S, LiBr

D. Use the information below to answer. (3 points)

property A b cMelting Point 801ºC -117ºC -39ºCBoiling Point 1456ºC 78ºC 357ºCWater Solubility yes yes noConductivity in the solid state

no no yes

Conductivity in the liquid state

yes no yes

Distorsion of the solid

brittle - yes

Sustance a has atoms joined by the type of bond called ________________________Sustance b has atoms joined by the type of bond called ________________________Sustance c has atoms joined by the type of bond called ________________________

E. Determine the type of bond, if there is any, according to the type of atoms (4 points)Type of Atoms Type of BondNa NaS ClBr CaFe Zn

F. Use Lewis diagrams to show the formation of the compound formed with carbonate (CO3-2) and

lithium. (3 points)

G. Use Lewis structure to show the formation of the compound formed with silicon and sulfide.(2pts)

H. Write the property of metals that is shown: (2 points)

_____________________________________________

____________________________________________________

Ionic Bonding and Ionic Bonds/ Metallic Bonding

1. Use Lewis diagrams to represent the formation of compounds that is formed from the elements selenium and sulfur and(b) write the symbol of the ions that form the compound illustrated in figure (b. Write formulas for each one. (c)

2. Write which compound is ionic and which is covalent or metallic:a) Compound X has a melting point of 1011 degrees Celcius and dissolves in water.

____________________b) Compound W is gaseous, does not conduct electricity and dissolves in water.

____________________c) d) NH4Cl_______________________

e)

__________________________ ______________________________

f) Tungsten_________________

g) It can be shaped into useful tools________________________

h) CN-______________________

3. Which has the highest crystal lattice energy: AIN or K3N. Explain

4. Put the following substances in decreasing order of their boiling points: explain.LiBr,N2,HCl,HBr,HF,RbBr._______________________________________

5. Use the noble gas electron configurations of atoms and ions to explain why when cobalt combines chemically whit oxygen it can form two types of ionic compounds, however

when cadmium combines chemically whit oxygen, one type of compound is formed. What are the ratios of the ions in each of the three compounds ?

6. Write what metallic property is illustrated:_______________________________

7. Three metals have the following melting points in kelvin: 1112,1814 and 336. Write the melting points in the corresponding place in the below:

State what happens to the strength of the metallic bond for these metals . Explain as fully as you can the effect you have described.

Geometría Molecular

Formula Dibujo de su geometría molecular

Nombre de la forma

Angulo (s) Polaridad de la molécula

SO3

H3O+

SeCl5I

H2O2

2. Dibuja la formula estructural de Lewis con su forma de la especie en la cual el átomo de nitrógeno esta unido a dos átomos de azufre y el ángulo es aproximadamente 180°.

Estructura de Lewis nombre de la forma

3. Predice cual tiene la propiedad más baja. ¿Por qué?

La solubilidad en agua del HF y el CS2 ____________________________

¿Por qué el CO2 es un gas y no un líquido bajo condiciones normales de temperatura y presión?

4. Predice todos los ángulos posibles en las moléculas.

________________________ ________________________

5. Prediga la hibridización de los átomos numerados

6. ¿Cuáles son las fuerzas intermoleculares que determinan las propiedades de cada compuesto?

____________________________________ _________________________________

____________________________________ _________________________________

___________________________________ _________________________________

Instituto Panamericano

Tercer trimestre: Taller de Química #4

Geometría Molecular

1. Completa la tabla:

FórmulaDibujo de su geometría molecular Nombre de la forma ángulo Polaridad de los enlaces

Polaridad de la molécula

SbH5

NbBr5

H3C2O2-

ONCl

C2H2

Cl2CO

N2O4

2. Dibuja la estructura de Lewis y luego la forma de la especie en la cual el átomo de nitrógeno está unido a dos átomos de azufre y el ángulo es aproximadamente 120ª.

Diagrama de Lewis geometría molecular nombre de la forma

3. Prediga que propiedad es la más baja en cada par. ¿Por qué?

a) El punto de fusión del agua o del cloruro de hidrógeno (HCl) _________________________________

b) El punto de fusión del CH4 o CHCl3 ___________________________________

4. Prediga todos los ángulos posibles en la molécula.

H O

R C C O H

N H

H

5.Prediga la hibridización de los átomos numerados:

CH CHCH CH=CHCH

CH

C1_____ C2_____ C3_____

6. ¿Cuáles de las siguientes fuerzas intermoleculares está incorrectamente asignada como la fuerza intermolecular principal del compuesto?

a) CH4 , London

b)NH3 , enlaces de hidrógeno

c) H2S, dipolo-dipolo

d) H3P, puentes de hidrógeno

e) AsH3 ,dipolo-dipolo

7. Los aminoácidos son los materiales básicos de las proteínas. Dos moléculas del aminoácido más simple a continuación. Dibuje los enlaces de hidrógeno entre ellos.

H H O H H O

N C C N C C

H H C H OH H H C H OH

H C H H C H

S S

H C H H C H

H H