2nd QUARTER EXAM NA!!!

Hi grade 9 GONZAGA, JOGUES, and REGIS!

I hope this site would help you guys. 

Exam coverage: 

Chapter 5: the periodic table

Chapter 6:er ionic trends

Chapter 7: ionic bonding

Chapter 8: covalent bonding

Chapter 9: chemical reactions

Enjoy studying!

XOXO

2015: BALANCING CHEMICAL EQUATIONS

Chapter 9: Chemical Reactions

Balancing Chemical Equations Worksheet

1. _____ Zn (s) + _____ AgNO₃ (aq) →  _____ Zn(NO₃)₂ (aq) + _____ Ag (s)

2. _____ N₂ (g) + _____ H₂ (g) → _____ NH₃ (g)

3. _____ NaCl (aq) + _____ AgC₂H₃O₂ (aq) → _____ NaC₂H₃O₂ (aq) + _____ AgCl (s)

4. _____ Mg(OH)₂ (aq) + _____ H₃PO₄ (aq) → _____ H₂O (l) + _____ Mg₃(PO₄ )₂ (aq)

5. _____ HNO₃ (aq) + _____ Ni (s) → _____ Ni(NO₃)₂ (aq) + _____ H₂ (g)

6. _____ Ba(HCO₃)₂ (s) → _____ BaCO₃ (s) + _____ H₂O (g) + _____ CO₂ (g)

7. _____ BaCl₂ (aq) + _____ Na₂SO₄ (aq) → _____ NaCl (aq) + _____ BaSO₄ (s)

8. _____ Al₂(CO₃)₃ (s) → _____ Al₂O₃ (s) + _____ CO₂ (g)

9. _____ Ca (s) + _____ H₂O (l) → _____ Ca(OH)₂ (aq) + _____ H₂ (g)

10. _____ LiHCO₃ (s) → _____ Li₂CO₃ (s) + _____ H₂O (g) + _____ CO₂(g)

11. _____ N₂ (g) + _____ O₂ (g) → _____ N₂O₅ (g)

12. _____ MgBr₂ (aq) + _____ KOH (aq) → _____ KBr (aq) + _____ Mg(OH)₂ (s)

13. _____ Mn (s) + _____ CuCl (aq) → _____ Cu (s) + _____ MnCl₂ (s)

14. _____ Zn (s) + _____ S₈ (s) → _____ ZnS (s)

15. _____ NaOH (aq) + _____ H₂SO₄ (aq) → _____ H₂O (l) + _____ Na₂SO₄ (aq)

16. _____ K (s) + _____ H₂O (l) → _____ KOH (aq) + _____ H₂ (g)

17. _____ C₅H₁₂ (l) + _____ O₂ (g) → _____ H₂O (g) + _____ CO₂ (g)

18. _____ KOH (aq) + _____ H₂CO₃ (aq) → _____ H₂O (l) + _____ K₂CO₃ (aq)

19. _____ C₄H₈O₂ (l) + _____ O₂ (g) → _____ H₂O (g) + _____ CO₂ (g)

20. _____ Al (s) + _____ S₈ (s) → _____ Al₂S₃ (s)

Answer: If it's balanced then you are right!

2015: NAMING MOLECULAR COMPOUNDS

Naming Molecular Compounds Worksheet

Write the names of the following covalent compounds:

21)       SO₃ __________________________________________

22)       N₂S __________________________________________

23)       PH₃ __________________________________________

24)       BF₃ __________________________________________

25)       P₂Br₄ __________________________________________

26)       CO __________________________________________

27)       SiO₂ __________________________________________

28)       SF₆ __________________________________________

29)       NH₃ __________________________________________

30)       NO₂ __________________________________________

Write the formulas of the following covalent compounds:

31)       nitrogen trichloride __________________________________________

32)       boron carbide __________________________________________

33)       dinitrogen trioxide __________________________________________

34)       phosphorus pentafluoride ______________________________________

35)       methane __________________________________________

36)       sulfur dibromide __________________________________________

37)       diboron tetrahydride __________________________________________

38)       oxygen difluoride __________________________________________

39)       carbon disulfide __________________________________________

40)       nitrogen monoxide __________________________________________

Answers:

Write the names of the following covalent compounds:

21)      SO₃                 sulfur trioxide

22)      N₂S                 dinitrogen sulfide

23)      PH₃                 phosphorus trihydride

24)      BF₃                 boron trifluoride

25)      P₂Br₄               diphosphorus tetrabromide

26)      CO                  carbon monoxide

27)      SiO₂                silicon dioxide

28)      SF₆                 sulfur hexafluoride

29)      NH₃                 ammonia

30)      NO₂                 nitrogen dioxide

Write the formulas of the following covalent compounds:

31)      nitrogen trichloride                          NCl₃

32)      boron carbide                                   BC

33)      dinitrogen trioxide                            N₂O₃

34)      phosphorus pentafluoride               PF₅

35)      methane                                            CH₄

36)      sulfur dibromide                               SBr₂

37)      diboron tetrahydride                        B₂H₄

38)      oxygen difluoride                             OF₂

39)      carbon disulfide                               CS₂

2015: NAMING IONIC COMPOUNDS

Naming Ionic Compounds Worksheet

Name the following ionic compounds:

1)         NaBr __________________________________________

2)         CaO __________________________________________

3)         Li₂S __________________________________________

4)         MgBr₂ __________________________________________

5)         Be(OH)₂ __________________________________________

Write the formulas for the following ionic compounds:

6)         potassium iodide __________________________________________

7)         magnesium oxide __________________________________________

8)         aluminum chloride __________________________________________

9)         sodium nitrate __________________________________________

10)       calcium carbonate __________________________________________

11)       lithium sulfate __________________________________________

12)       beryllium phosphide __________________________________________

13)       magnesium hydroxide _________________________________________

14)       sodium phosphate __________________________________________

15)       aluminum carbonate __________________________________________

16)       calcium chloride __________________________________________

17)       sodium cyanide __________________________________________

18)       aluminum oxide __________________________________________

19)       magnesium acetate __________________________________________

20)       ammonium chloride __________________________________________

Answers: 

Name the following ionic compounds:

1)         NaBr                           sodium bromide

2)         CaO                            calcium oxide

3)         Li₂S                             lithium sulfide

4)         MgBr₂                         magnesium bromide

5)         Be(OH)₂                     beryllium hydroxide

Write the formulas for the following ionic compounds:

6)         potassium iodide                 KI

7)         magnesium oxide                MgO

8)         aluminum chloride              AlCl₃

9)         sodium nitrate                      NaNO₃

10)      calcium carbonate               CaCO₃

11)      lithium sulfate                      Li₂SO₄

12)      beryllium phosphide           Be₃P₂

13)      magnesium hydroxide        Mg(OH)₂

14)      sodium phosphate              Na₃PO₄

15)      aluminum carbonate          Al₂(CO₃)₃

16)      calcium chloride                  CaCl₂

17)      sodium cyanide                   NaCN

18)      aluminum oxide                   Al₂O₃

19)      magnesium acetate            Mg(C₂H₃O₂)₂

20)      ammonium chloride            NH₄Cl

  

2015: CHEMICAL BONDING

CHEMICAL BONDING

1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom.

A) 4, 2

B) 2, 4

C) 2, 3

D) 4, 3

E) 0, 3 

 

2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.

A) 4, 2

B) 4,1

C) 2, 5

D) 6, 1

E) 0, 5 

 

3) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

A) 7, 4, and 6

B) 1, 5, and 7

C) 8, 2, and 3

D) 7, 1, and 2

E) 2, 7, and 4 

4) The only noble gas without eight valence electrons is __________.

A) Ar

B) Ne

C) He

D) Kr

E) All noble gases have eight valence electrons.

5) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration?

             O        Sr        Na        Se        Br

A) O, Se

B) Sr

C) Na

D) Br

E) Sr, O, Se

6) Elements from opposite sides of the periodic table tend to form __________.

A) covalent compounds

B) ionic compounds

C) compounds that are gaseous at room temperature

D) homonuclear diatomic compounds

E) covalent compounds that are gaseous at room temperature

7) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?

A) 3

B) 4

C) 1

D) 2

E) 0

8) What is the maximum number of double bonds that a hydrogen atom can form?

A) 0

B) 1

C) 2

D) 3

E) 4

9) The ability of an atom in a molecule to attract electrons is best quantified by the __________.

A) paramagnetism

B) diamagnetism

C) electronegativity

D) electron change-to-mass ratio

E) first ionization potential

10) Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

A) decreases, increases

B) increases, increases

C) increases, decreases

D) stays the same, increases

E) increases, stays the same

11) The type of compound that is most likely to contain a covalent bond is __________.

A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table

B) a solid metal

C) one that is composed of only nonmetals

D) held together by the electrostatic forces between oppositely charged ions

E) There is no general rule to predict covalency in bonds.

12) Of the atoms below, __________ is the most electronegative.

A) Br

B) O

C) Cl

D) N

E) F

13) Of the atoms below, __________ is the least electronegative.

A) Rb

B) F

C) Si

D) Cl

E) Ca

14) Which of the following names is/are correct for the compound TiO2?

A) titanium dioxide and titanium (IV) oxide

B) titanium (IV) dioxide

C) titanium oxide

D) titanium oxide and titanium (IV) dioxide

E) titanium (II) oxide

15) The Lewis structure of N2H2 shows __________.

A) a nitrogen-nitrogen triple bond

B) a nitrogen-nitrogen single bond

C) each nitrogen has one nonbonding electron pair

D) each nitrogen has two nonbonding electron pairs

E) each hydrogen has one nonbonding electron pair

Answers: cddcb   bbacc   ceaac

PERIODIC TRENDS 2018

PERIODIC TABLE AND PERIODIC TRENDS PART 

Matching

Match each item with the correct statement below.

a.	group	d.	metal
b.	ionization energy	e.	periodic law
c.	atomic radius

____    1.   vertical column in the periodic table

____    2.   A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____    3.   type of element that is a good conductor of heat and electric current

____    4.   one-half the distance between the nuclei of two atoms when the atoms are joined; size of the atom

____    5.   energy required to remove an electron from an atom

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____    6.   What is another name for the transition metals?

a.	noble gases	c.	Group B elements
b.	Group A elements	d.	Group C elements

____    7.   Which of the following elements is in the same period as phosphorus?

a.	carbon	c.	nitrogen
b.	magnesium	d.	oxygen

____    8.   Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?

a.	Henry Moseley	c.	John Dalton
b.	Antoine Lavoisier	d.	Dmitri Mendeleev

____    9.   Which of the following categories includes the majority of the elements?

a.	metalloids	c.	metals
b.	liquids	d.	nonmetals

____  10.   Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a.	Pt	c.	Li
b.	V	d.	Kr

____  11.   In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a.	In, 49 protons, 49 electrons	c.	Cs, 55 protons, 132.9 electrons
b.	Zn, 30 protons, 60 electrons	d.	F, 19 protons, 19 electrons

____  12.   What element has the electron configuration 1s2s2p3s3p2?

a.	nitrogen	c.	silicon
b.	selenium	d.	silver

____  13.   Which of the following is true about the electron configurations of the noble gases?

a.	The highest occupied s and p sublevels are completely filled.
b.	The highest occupied s and p sublevels are partially filled.
c.	The electrons with the highest energy are in a d sublevel.
d.	The electrons with the highest energy are in an f sublevel.

____  14.   Which subatomic particle plays the greatest part in determining the properties of an element?

a.	proton	c.	neutron
b.	electron	d.	none of the above

____  15.   Which of the following elements is a main transition metal?

a.	cesium	c.	tellurium
b.	copper	d.	tin

____  16.   Which of the following groupings contains only representative elements?

a.	Cu, Co, Cd	c.	Al, Mg, Li
b.	Ni, Fe, Zn	d.	Hg, Cr, Ag

____  17.   What is another name for Group 1A?

a.	alkali metals	c.	noble gases
b.	alkaline earth metals	d.	halogens

____  18.   Of the elements Fe, Sn, U, and Br, which is a halogen?

a.	Fe	c.	U
b.	Sn	d.	Br

____  19.   How does atomic radius change from top to bottom in a group in the periodic table?

a.	It tends to decrease.	c.	It first increases, then decreases.
b.	It tends to increase.	d.	It first decreases, then increases.

____  20.   How does atomic radius change from left to right across a period in the periodic table?

a.	It tends to decrease.	c.	It first increases, then decreases.
b.	It tends to increase.	d.	It first decreases, then increases.

____  21.   What causes the shielding effect to remain constant across a period?

a.	Electrons are added to the same principal energy level.
b.	Electrons are added to different principal energy levels.
c.	The charge on the nucleus is constant.
d.	The atomic radius increases.

____  22.   What element in the second period has the largest atomic radius?

a.	carbon	c.	potassium
b.	lithium	d.	neon

____  23.   Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?

a.	more shielding of the electrons by the highest occupied energy level
b.	an increase in size of the nucleus
c.	an increase in number of protons
d.	fewer electrons in the highest occupied energy level

____  24.   What is the charge of a cation?

a.	a positive charge
b.	no charge
c.	a negative charge
d.	The charge depends on the size of the nucleus.

____  25.   Which of the following statements is true about ions?

a.	Cations form when an atom gains electrons.
b.	Cations form when an atom loses electrons.
c.	Anions form when an atom gains protons.
d.	Anions form when an atom loses protons.

____  26.   The metals in Groups 1A, 2A, and 3A ____.

a.	gain electrons when they form ions	c.	all have ions with a 1+ charge
b.	all form ions with a negative charge	d.	lose electrons when they form ions

____  27.   Which of the following statements is NOT true about ions?

a.	Cations are positively charged ions.
b.	Anions are common among nonmetals.
c.	Charges for ions are written as numbers followed by a plus or minus sign.
d.	When a cation forms, more electrons are transferred to it.

____  28.   In which of the following sets are the charges given correctly for all the ions?

a.	Na+, Mg+, Al+	c.	Rb-, Ba+2, P+3
b.	K+, Sr+2, O-2	d.	N-, O-2, F+3

____  29.   What is the element with the highest electronegativity value?

a.	cesium	c.	calcium
b.	helium	d.	fluorine

____  30.   Which of the following elements has the smallest ionic radius?

a.	Li	c.	O
b.	K	d.	S

____  31.   Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?

a.	increase in atomic size
b.	increase in size of the nucleus
c.	increase in number of protons
d.	fewer electrons in the highest occupied energy level

____  32.   Which of the following elements has the smallest first ionization energy?

a.	sodium	c.	potassium
b.	calcium	d.	magnesium

____  33.   Which statement is true about electronegativity?

a.	Electronegativity is the ability of an anion to attract another anion.
b.	Electronegativity generally increases as you move from top to bottom within a group.
c.	Electronegativity generally is higher for metals than for nonmetals.
d.	Electronegativity generally increases from left to right across a period.

____  34.   As you move from left to right across the second period of the periodic table ____.

a.	ionization energy increases	c.	electronegativity decreases
b.	atomic radii increase	d.	atomic mass decreases

____  35.   Of the following elements, which one has the smallest first ionization energy?

a.	boron	c.	aluminum
b.	carbon	d.	silicon Answers:  aedcb   ccdcd   acabb   cadba   abaab   ddbdc   acdac  How well did you do? Tell me about it. :)