CHEM151 Week 3

A potassium atom LOSES ONE ELECTRON to form a

+ 1 ion.

A sulfur atom GAINS TWO ELECTRONS to form a

- 2 ion.

An atom or ion has 43 neutrons, 36 protons, and 36 electrons. Determine charge for this atom or ion.

0

How many moles of argon are in 31.5 g of argon? *******

0.789

How many oxygen atoms are present in each of the formulas? C(lower 4)H(lower 8)O

1

Calculate the formula mass of each compound. Keep at least one decimal place in atomic masses from the periodic table. Water, H(lower 2) O

18.015 amu

Calculate the formula mass of calcium bromite, Ca(BrO)(lower 2)lower 2

263.8836 amu

How many total electrons are in a Cu(upper 2+) ion?

27

An ion has a mass number of 65, 36 neutrons, and a charge of + 1. Determine the number of electrons in this ion.

28

An ion has a mass number of 65, 36 neutrons, and a charge of + 1. Determine the number of protons in this ion.

29

How many oxygen atoms are present in each of the formulas? H(lower 2)SO(lower 3)

3

A bucket of nails contain 408 nails. How many dozens of nails does the bucket contain?

34

Identify the missing information for each atom or ion. Note that the atoms and ions are not necessarily neutral. A Se ion has a mass number of 78 and a charge of - 2. Determine the number of protons in this ion.

34

Identify the missing information for each atom or ion. Note that the atoms and ions are not necessarily neutral. A Se ion has a mass number of 78 and a charge of - 2. Determine the number of electrons in this ion.

36

Identify the missing information for each atom or ion. Note that the atoms and ions are not necessarily neutral. A Se ion has a mass number of 78 and a charge of - 2. Determine the number of neutrons in this ion.

44

Determine the number of K(+upper) and F(-lower) ions required to form a neutral ionic compound. ****

5 K(+upper) 5 F(-upper)

How many protons are in an atom with 54 electrons and a - 1 charge?

53 protons

An atom or ion has 43 neutrons, 36 protons, and 36 electrons. Determine the mass number.

79

Calculate the formula mass of each compound. Keep at least one decimal place in atomic masses from the periodic table. Phosphoric Acid H(lower 3)PO(lower 4)

98.00 amu

Determine the chemical formula for each of the compounds. silver sulfate

Ag(lower 2)SO(lower 4)

Caroline knows the amount of a compound in moles. To find the number of molecules in the given sample of her compound, what values must also be used in her calculation?

Avogadro's number

What is the name of the compound with the chemical formula BaI (lower 2)

Barium Iodide

What is the name of the compound with the chemical formula BaS?

Barium sulfide

One molecule of caffeine contains 8 atoms of carbon, 10 atoms of hydrogen, 4 atoms of nitrogen, and 2 atoms of oxygen. Write the formula for caffeine with the elements in the order that they are given.

C(lower 8)H(lower 10)N(lower 4)O(lower 2)

Determine the empirical formula for each compound from the molecular formula. C(lower 4) H( lower 8)

CH(lower 2)

Determine the empirical formula for each compound from the molecular formula. C(lower 2)H(lower 4) O(lower 2)

CH(lower 2)O

Determine the formula for each compound or element. calcium chlorate

Ca(ClO lower 3)lower 2

Determine the formula for each compound or element. calcium chloride

CaCl(lower 2)

What is an ionic compound?

Consists of a metal and nonmetal

What is a molecular compound?

Consists of two nonmetals

Give the systematic name of each of the compounds. CuBr

Copper(I)bromide

Determine the chemical name of the ionic compound formed from the ions Cu(upper 2+) and NO(upper - 3)

Copper(II) nitrate

Enter the formula for the ionic compound. chromium(II) oxide

CrO

An ion has a mass number of 65, 36 neutrons, and a charge of + 1. Identify the element symbol.

Cu

Determine the chemical formula of the ionic compound formed from the ions Cu(upper 2+) and NO(upper - 3)

Cu(NO lower 3) lower 2

Do these 3 chemical formulas represent empirical or not empirical formulas? NaCl, PF(lower 3), CO(lower 2) . ***

Empirical Formulas

Enter the formula for the ionic compound. iron (III) sulfide

Fe(lower 2)S(lower 3)

Give the systematic name of each of the compounds. Au(lower 2)S(lower 3)

Gold (III)sulfide

Some of the formulas could be either molecular or empirical formulas, however, some can only be molecular formulas? Name two that must be molecular formulas. ****

H(lower 2) O (lower 2) C(lower 4) H(lower 8) O(lower 4)

Name the compound. HF(aq)

Hydrofluoric acid

Give the systematic name of each of the compounds. FeCl (lower 2)

Iron(II)chloride

What is a molecular formula? ***

It gives the number of atoms of each of the elements present in one molecule of a specific compound.

Determine the formula for potassium sulfide.

K(lower 2)S

Determine the chemical formula for each of the compounds. potassium phosphate

K(lower 3)PO(lower 4)

An atom or ion has 43 neutrons, 36 protons, and 36 electrons. Identify the element symbol.

Kr

Give the systematic name of each of the compounds. PbO(lower 2)

Lead(IV)oxide

Enter the formula for the ionic compound. manganese (II) chloride

MnCl (lower 2)

What do these 3 statements describe? The amount of a substance containing the same number of formula units as there are atoms in 12 g of carbon. 6.022 x 10 (23rd power) items. Avogadro's number of items

Mole

Determine the chemical formula for each of the compounds. ammonium nitrate

NH(lower 4)NO(lower 3)

Some of the formulas could be either molecular or empirical formulas, however, some can only be molecular formulas? Name three that are not molecular formulas. ****

NO(lower 2) HO C(lower 3) H(lower 4) O (lower 3)

What is the simplest formula for a compound that contains 0.50 mol Na, 0.50 mol S, and 0.75 mol O?

Na(lower 2)S(lower 2)O(lower 3)

Determine the chemical formula for each of the compounds. sodium sulfite

Na(lower 2)SO(lower 3)

Enter the formula for the ionic compound. sodium nitride

Na(lower 3)N

Name 2 ionic compounds

NaBr FeCl(lower 3)

Name two ionic compounds. #3 of 7 ?'s Q#2

NaBr Q#2 FeCl (lower 3)

What is the name of the ion? NO(lower 2)

Nitrite

Do these 3 chemical formulas represent empirical or not empirical formulas? C(lower 6) H(lower 12) O(lower 6) H(lower 2) O(Lower 2) C(lower 4) H(lower 8) . ****

Not Empirical Formulas

Determine the formula for each compound or element. oxygen gas

O(lower 2)

Name 2 molecular compounds.

SO(lower 2) NCl (lower 3)

Name two molecular compounds #3 of 7 ?'s Q#2

SO(lower 2) Q#2 CH(lower 4)

Select the pair of elements you would expect to have similar properties. ***

Si and Ge

Name the compound. Na(lower 2)SO(lower 4)

Sodium sulfate

Write the name of the compound with the chemical formula SO(lower 2).

Sulfur Dioxide

Name the compound. SO(lower 2)

Sulfur dioxide

Which definition best describes the term molar mass?

The mass, in grams, of one mole of a substance

What is an empirical formula? ***

The simplest positive integer ratio of atoms present in a compound. A simple example of this concept is that the empirical formula of sulfur monoxide, or SO, would simply be SO, as is the empirical formula of disulfur dioxide, S(lower 2)O(lower 2).

Label the 2 far left and 2 far right categories in the periodic table.

alkali metals, alkaline earth metals, halogens, noble gases