Question 1

Groups—Columns:Groups are the columns of the periodic table

Accepted Answer

Groups are the columns of the periodic table

Question 2

The five groups are known by name:

Accepted Answer

Group                      Name                                                                  Elements1A                                 Alkali metals                                                 Li, Na, K, Rb, Cs, Fr

Question 3

The five groups are known by name:

Accepted Answer

Group                      Name                                                                  Elements2A                               Alkaline earth metals                            Be, Mg, Ca, Sr, Ba, Ra

Question 4

The five groups are known by name:

Accepted Answer

Group                      Name                                                                  Elements6A                               Chalcogens                                                   O, S, Se, Te, Po

Question 5

The five groups are known by name:

Accepted Answer

Group                      Name                                                                  Elements7A                                Halogens                                                          F, Cl, Br, I, At

Question 6

The five groups are known by name:

Accepted Answer

Group                      Name                                                                  Elements8A                                Noble gases                                                  He, Ne, Ar, Kr, Xe, Rn

Question 7

Periodic Table (1 of 3):Metals are on the left side of the periodic table.

Accepted Answer

Some properties of metals include: • Shiny luster • Conducting heat and electricity • Solids (except mercury)

Question 8

Example of some metals

Accepted Answer

Iron (Fe)Copper (Cu)Aluminum (AI)Silver (Ag)Lead (Pb)Gold (Au)

Question 9

Periodic Table (2 of 3):Nonmetals are on the right side of the periodic table (they include H).

Accepted Answer

They can be solid (like carbon), liquid (like bromine), or gas (like neon) at room temperature.

Question 10

Examples of some nonmetals

Accepted Answer

Bromine (Br)Carbon (C)Sulfur (S)Phosphorus (P)

Question 11

Periodic Table (3 of 3)Elements on the steplike purple line are metalloids (except Al, Po, and At).

Accepted Answer

Their properties are sometimes like metals and sometimes like nonmetals.

Question 12

Molecules and Molecular Compounds

Accepted Answer

Chemical FormulaMolecular compounds

Question 13

Chemical Formula

Accepted Answer

The subscript to the right of the symbol of an element tells the number of atoms of that element in one molecule of the compound.

Question 14

Molecular compounds

Accepted Answer

They are composed of molecules and almost always contain only nonmetals.

Question 15

Diatomic MoleculesThese seven elements occur naturally as molecules containing two atoms:

Accepted Answer

• Hydrogen ($$H_{_2}$$)• Nitrogen ($$N_{_2}$$)• Oxygen ($$O_{_2}$$)• Fluorine ($$F_{_2}$$)• Chlorine ($$CI_{_2}$$)• Bromine ($$Br_{_2}$$)• Iodine ($$I_{_2})$$Note their location on the periodic table

Question 16

Types of Formulas

Accepted Answer

Empirical formulasMolecular formulas

Question 17

Empirical formulas

Accepted Answer

give the lowest whole-number ratio of atoms of each element in a compound.If we know the molecular formula of a compound, we can determine its empirical formula. The converse is not true without more information.

Question 18

Molecular formulas

Accepted Answer

give the exact number of atoms of each element in a compound.If we know the molecular formula of a compound, we can determine its empirical formula. The converse is not true without more information.

Question 19

Picturing Molecules (#38)Structural formulas (2D)

Accepted Answer

show the order in which atoms are attached. They do NOT depict the three-dimensional (3D) shape of molecules.

Question 20

Perspective drawings, ball-and-stick models, and space-filling models

Accepted Answer

show the three-dimensional (3D) order of the atoms in a compound.

Question 21

Ions and Ionic Compounds (#39)When an atom of a group of atoms loses or gains electrons, it becomes an ion.

Accepted Answer

CationsAnions

Question 22

Cations

Accepted Answer

Cations are formed when at least one electron is lost. Monatomic cations are formed by metals.

Question 23

Anions

Accepted Answer

Anions are formed when at least one electron is gained. Monatomic anions are formed by nonmetals, except the noble gases.

Question 24

Ionic CompoundsIonic compounds

Accepted Answer

Ionic compounds (such as NaCl) are generally formed between metals and nonmetals.Electrons are transferred from the metal to the nonmetal. The oppositely charged ions attract each other. Only empirical formulas are written.

Question 25

Naming Inorganic CompoundsThe system of naming compounds is called chemical nomenclature.

Accepted Answer

• Names of ions (cations and anions) must be memorized• There are rules used to name: 1) Ionic compounds 2) Acids 3) Binary molecular compounds

Question 26

Common Cations (#42)Namehydrogen ion

Accepted Answer

Formula$$H^{+}$$Charge$$1^{+}$$

Question 27

Namesodium ion

Accepted Answer

Formula$$Na^{+}$$Charge $$1^{+}$$,

Question 28

Namepotassium ion

Accepted Answer

Formula$$K^{+}$$Charge $$1^{+}$$

Question 29

Namesilver ion

Accepted Answer

Formula$$Ag+$$Charge $$1^{+}$$

Question 30

Nameammonium ion

Accepted Answer

Formula$$NH_{_4}^{+}$$Charge$$1^{+}$$

Question 31

Namemagnesium ion

Accepted Answer

Formula $$Mg^{2+}$$ Charge$$2^{+}$$

Question 32

Namecalcium ion

Accepted Answer

Formula $$Ca^{2+}$$Charge$$2^{+}$$

Question 33

Namezinc ion

Accepted Answer

Formula $$Zn^{2+}$$Charge$$2^{+}$$

Question 34

Namecopper (II) or cupric ion

Accepted Answer

Formula $$Cu^{2+}$$Charge$$2^{+}$$

Question 35

Name iron (II) or ferrous ion

Accepted Answer

Formula $$Fe^{2+}$$Charge$$2^{+}$$

Question 36

Namelead (II) or plumbous ion

Accepted Answer

Formula $$Pb^{2+}$$Charge$$2^{+}$$

Question 37

Common Anions (#43)Namefluoride ion

Accepted Answer

Formula $$F^{-}$$Charge$$1^{-}$$

Question 38

Name chloride ion

Accepted Answer

Formula$$CI^{-}$$Charge $$1^{-}$$

Question 39

Namebromide ion

Accepted Answer

Formula $$Br^{-}$$Charge$$1^{-}$$

Question 40

Nameiodide ion

Accepted Answer

Formula $$I^{-}$$Charge$$1^{-}$$

Question 41

Namehydroxide ion

Accepted Answer

Formula $$OH^{-}$$ Charge$$1^{-}$$

Question 42

Nameacetate ion

Accepted Answer

Formula $$CH_{_3}COO^{-} or$$ $$C_{_2}H_{_3}O_{_2}^{-}$$Charge$$1^{-}$$

Question 43

Nameperchlorate ion

Accepted Answer

Formula $$CIO_{_4}^{-}$$Charge$$1^{-}$$

Question 44

Namenitrate ion

Accepted Answer

Formula $$NO_{_3}^{-}$$Charge$$1^{-}$$

Question 45

Name sulfide ion

Accepted Answer

Formula $$S^{2_{}-}$$Charge$$2^{-}$$

Question 46

Namecarbonate ion

Accepted Answer

Formula$$CO_{_3}^{2-}$$ Charge$$2^{-}$$

Question 47

Namesulfate ion

Accepted Answer

Formula $$SO_{_4}^{2-}$$Charge$$2^{-}$$

Question 48

Namephosphate ion

Accepted Answer

Formula $$PO_{_4}^{3-}$$ Charge$$3^{-}$$

Question 49

Polyatomic IonsSometimes a group of atoms will gain or lose electrons. These are polyatomic ions.

Accepted Answer

A polyatomic cation: Ammonium ≡ $$NH_{_4}^{+}A $$polyatomic anion: Sulfate ≡ $$SO_{_4}^{2-}$$

Question 50

Writing Inorganic Formulas Because compounds are electrically neutral, one can determine the formula of a compound this way:

Accepted Answer

⁃ The charge on the cation becomes the subscript on the anion. ⁃ The charge on the anion becomes the subscript on the cation. ⁃ If these subscripts are not in the lowest whole-number ratio, divide them by the greatest common factor.

Question 51

Reference PowerPoint #45

Accepted Answer

$$Mg^{2+}$N^{3-}$$= $$Mg_{_3}^{}N_{_2}^{}$$

Question 52

Naming Inorganic Compounds• The cation is named before the anion.

Accepted Answer

Write the element name of the cation.

Question 53

If the cation can have more than one possible charge, write the charge as a Roman numeral in parentheses, i.e. for iron:

Accepted Answer

$$Fe^{2+} is $$iron (II), $$Fe^{3+} is $$iron (III).

Question 54

If it is a polyatomic cation

Accepted Answer

If it is a polyatomic cation, it will end in –ium, i.e., $$NH_{_4}^{+} is $$ammonium

Question 55

If the element is the anion

Accepted Answer

If the element is the anion, change its ending to –ide, i.e., $$CI^{-} is $$chloride

Question 56

If the anion is a polyatomic ion

Accepted Answer

If the anion is a polyatomic ion, simply write the name of the polyatomic ion, i.e., $$PO_{_4}^{3-_{}}is $$phosphate.

Question 57

Patterns in Oxyanion Nomenclature (1 of 3)When there are only two oxyanions involving the same element:

Accepted Answer

The one with fewer oxygens ends in -ite.$$NO_{_2}^{-} is $$nitrite$$NO_{_3}^{-} is $$nitrateThe one with more oxygens ends in -ate.$$SO3^{2-} is $$sulfite$$SO4^{2-} is $$sulfate

Question 58

Patterns in Oxyanion Nomenclature (2 of 3)(#48)Central atoms on the second row have a bond to, at most, three oxygens; those on the third row take up to four.

Accepted Answer

Ion charges decrease as you go from left to right.

Question 59

Patterns in Oxyanion Nomenclature (3 of 3) (#49)The ion with two oxygens:

Accepted Answer

The ion with two oxygens ends in -ite: $$CIO_{_2}^{-} is $$chlorite.

Question 60

The ion with three oxygens:

Accepted Answer

The ion with three oxygens ends in -ate: $$CO_{_3}^{-}is $$chlorate.

Question 61

The ion with one oxygen:

Accepted Answer

The ion with one oxygen has the prefix hypo- and ends in -ite: $$CIO^{-} is $$hypochlorite

Question 62

The ion with four oxygens:

Accepted Answer

The ion with four oxygens has the prefix per- and ends in -ate:  $$CIO_4^{-} is $$perchlorate.

Question 63

Inorganic Acid Nomenclature (#50)If the anion of the acid ends in -ide, change the ending to -ic acid and add the prefix hydro-

Accepted Answer

HCl: hydro chloric adci HBr: hydro bromic acid HI: hydro iodic acid

Question 64

If the anion ends in -ite, change the ending to -ous acid.

Accepted Answer

HClO: hypochlorous acid$$HCIO_{_2}$$: chlorous acid

Gen Chem 1 Exam 2 Chapter 2 (Flashcard deck 2)

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