Definitions, Laws, And Nomenclature Rules

Front 1

Dalton's Atomic Theory

Back 1

1. elements are made of tiny particles called atoms
2. all atoms of a given element are identical
3. the atoms of a given element are different from those of any other element.
4. atoms of one element can combine with atoms of other elements to form compounds. a given compound always has the same relative numbers and types of atoms.
5. atoms are indivisible in chemical processes. that is, atoms are not created nor destroyed in chemical rxns. a chemical rxn simply changes the way the atoms are grouped together

Front 2

law of constant composition

Back 2

a given compound always has the same composition, regardles or where it comes from.

Front 3

compound

Back 3

a distinct substance that is composed of the atoms of two or more elements and always contains exactly the same relative masses of those elements -- this simply means that a compound always contains the same relative numbers of atoms of each element.

Front 4

all atoms of the same element have the same number of ______ (the element's atomic number) and the same number of ______

Back 4

1. protons +
2. electrons -

Front 5

if a free atom, the positive and negative charges always balance to yield a net ____ charge

Back 5

zero

Front 6

def. or atomic number

Back 6

the number of protons (located at the top) also known as the "Z"

Front 7

def. of mass number

Back 7

the sum of protons and neutrons. also known as "A"

Front 8

def. of isotopes

Back 8

atoms with the same number or protons but diff. numbers of NEUTRONS.

Front 9

group 7A elements are called ______

Back 9

halogens

Front 10

group 8 elements are called _____

Back 10

noble gases.

Front 11

characteristics of metals

Back 11

1. efficient conduction of heat and electricity
2. malleability (they can be hammered into thin sheets)
3. ductility (they can be pulled into wires)
4. a lustrous (shiny) appearance

Front 12

def. of molecule

Back 12

a collection of atoms that behaves as a unit. molecules are always electrically neutral (zero charge)

Front 13

def. diatomic molecules

and name these elements

Back 13

1. molecules made up of two atoms.

2. hydrogen (H2), Nitrogen (N2), Oxygen (O2), Flourine (F2), Chlorine (Cl2), Bromine (Br2), Iodine (I2)

Front 14

name the physical states of hte following elements:

1.Hydrogen, 2. Nitrogen, 3. Oxygen, 4. Flourine, 5. Chlorine, 6. Bromine, 7. Iodine

Back 14

1. gas, 2. gas, 3. gas, 4. gas, 5. gas, 6. liquid, 7. solid

Front 15

def. of cation

Back 15

a positive ion produced when one or more electrons are LOST from a neutral atom. the size decreases when an atom loses one or more electrons

Front 16

def. of anion

Back 16

a negatively charged ion formed when electrons are GAINED by a neutral atom. the size increases when an atom gains one or more electrons to form a negative ion.

Front 17

naming of anions?

Back 17

the name of an anion is obtained by adding -ide to the root of the atom name. eg: Cl- (chlorine) is now called chloride ion

Front 18

for groups 1, 2, and 3, the charges of the cations equal the group numbers

Back 18

eg: group 1A = K+
group 2A = Ca2+
group 3A = Al 3+

Front 19

a substance containing ions that can move can conduct an ________

Back 19

electrical current

Front 20

an __________ cannot contain only anions or only cations, because the net charge of a compound must be zero

Back 20

ionic compound. a chem. compound must have a net charge of zero. - this means there must be both positive (cation) and negative ions (anions) present in a compound. so that they have a net charge or zero.

Front 21

def. or ionic compounds

Back 21

whenever a compound forms between a metal and a non metal, it can be expected to contain ions. we call these ionic compounds.

Front 22

binary compounds

Back 22

compounds composed of two elements

1. compounds that contain a metal and a nonmetal

2. compounds that contain two nonmetals

Front 23

binary ionic compounds

Back 23

contain a cation, which is always written FIRST in the formula, and an anion.

Front 24

give the name or each cation and anion

1. H+ , Li + Ag+

2. H-, F-, Cl-, Br-, I-, O2-, S2-

Back 24

1. hydrogen, lithium, silver

2. hydride, flouride, chloride, bromide, iodide, oxide, sulfide

remember: a simple cation has the same name as its parent element*

Front 25

rules for naming ionic compounds

Back 25

1. cation ALWAYS first and anion second.

2. a simple cation (single atom) takes its name from the name of the element. eg: Na+ = sodium
3. a simple anion (from a single atom) is named by taking the first part of the element name (the root) and adding -ide. thus the Cl- ion is called chloride

Front 26

give the names of the following compounds:

1. NaCl
2. KI
3. CaS
4. CsBr
5. MgO

Back 26

1. sodium chloride
2. potassium iodide
3. calcium sulfide
4. cesium bromide
5. magnesium oxide

Front 27

Type II binary IONIC compounds contain a metal that can from more than one type of cation. remember these rules:

Back 27

1. compounds formed from metals and nonmentals are ionic

2. in an ionic compound the cation is always named first

3. the net charge is always zero.

** because the cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses.

Front 28

give the systematic name of each of the following compounds:

1. CuCl

2. HgO

3. Fe2O3

4. MnO2

5. PbCl4

Back 28

1. copper (I) chloride

2. mercury (II) oxide

3. iron (III) oxide

4. manganese (IV) oxide

5. lead (IV) chloride

Front 29

rules for naming covalent (nonmetals only) compounds

Back 29

1. the first element in the formula is named first, and the full element name is used.

2. the second element is named as though it were an anion (ending with -ide)

3. prefixes are used to denot the numbers of atoms present.

4. mono- is never used for naming the first element.

Front 30

state the names of the following:

1. PCl5
2. P4O6
3. SF6
4. SO3
5. SO2
6. N2O3

Back 30

1. phosphorus pentachloride
2. tetraphosphorus hexoxide
3. sulfur hexafluoride
4. sulfur trioxide
5. sulfur dioxide
6. dinitrogen trioxide

Front 31

inic compounds containing _________ ions are not binary compounds because they contain more than two elements

Back 31

polyatomic ions

Front 32

give the systematic name of each of the following compounds

1. Na2SO4
2. KH2PO4
3. Fe(NO3)3
4. Mn(OH)2
5. Na2SO3
6. NH4ClO3

Back 32

1. sodium sulfate
2. potassium dihydrogen phosphate
3. iron (III) nitrate
4. manganese (II) hydroxide
5. sodium sulfite
6. ammonium chlorate

Front 33

name the following compounds:

1. CsClO4
2. FeBr3
3. PCl3
4. CuSO4

Back 33

1. cesium perchlorate

2. iron (III) bromide

3. phosphorus trichloride (both P and Cl are nonmetals!!!) make sure you check if they are metals or nonmetals first**

4. copper (II) sulfate

Front 34

def. acids

Back 34

certain molecules produce H+ ions (protons) when dissolved in water. these substances are called acids.

see rules**

Front 35

rules for naming acids

Back 35

1. if the anion does not contain oxygen (hydrogen is always the cation so the formula of an acid is always balanced) add the prefix hydro- and end with ic attaced.

2. if anion contains oxygen, add either -ic or -ous. when the anion name ends in -ate, the suffix -ic is used. and when anion name ends in -ite, the suffix -ous is used.

Front 36

name the following acids:

1. HClO4
2. HClO3
3. HClO2
4. HClO3

Back 36

1. perchlorate to perchloric acid

2. chlorate to chloric acid

3. chlorite to chlorous acid

4. hypochlorite to hypochlorous acid

Front 37

give the formula for the following compounds :

1. potassium hydroxide

2. sodium carbonate

3. nitric acid

4. cobalt (III) nitrate

5. calcium chloride

6. lead (IV) oxide

7. dinitrogen pentoxide

8. ammonium perchlorate

Back 37

1. KOH

2. Na2CO3

3. HNO3

4. Co(NO3)3

5. CaCl2

6. PbO2

7. N2O5

8. NH4ClO4

Front 38

clues that shows that chemical reaction has occured?

Back 38

color change, solid forms, bubbles form, and heat/flame is produced or heat is absorbed.