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Sec 5 Chemistry Dawson College > Test 1 > Flashcards

Test 1 Flashcards

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1
Q

What is chemistry?

A

Chemistry is the science that studies the composition, properties, and activity of matter.

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2
Q

What is matter?

A

Matter is the grouping of everything that constitutes life.

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3
Q

How does chemistry play into matter?

A

Chemistry allows us to study and understand matter and energy as well as the interaction between the different forms of matter.

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4
Q

What is an atom?

A

An atom is the smallest part of an element.

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5
Q

What are the atoms subatomic particles called?

A

Electrons, protons and neutrons.

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6
Q

What are the characteristics of electrons?

A

Tiny, very light particles, negative electrical charge, we neglect the mass because its too small.

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7
Q

What are the characteristics of protons?

A

Much larger and heavier then electrons, have a positive charge.

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8
Q

What are the characteristics of neutrons?

A

Large and heavy like protons, have no electrical charge.

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9
Q

Where are the protons located in the atom?

A

The nucleus

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10
Q

Where are the neutrons located in the atom?

A

The nucleus inbetween the protons to prevent them from repelling eachother.

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11
Q

Where are the electrons located in the atom?

A

The environment surrounding the nucleus and are in constant motion.

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12
Q

What is the function of a proton?

A

It helps to balance the negative charge of the electon.

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13
Q

What is the function of a neutron?

A

To prevent the positive charges of the protons from touching eachother.

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14
Q

What is the function of a electron?

A

The transfer of electrons is what causes all chemical reactions.

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15
Q

What is the atomic mass?

A

The atomic mass is the mass of the protons + the mass of the neutrons.

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16
Q

What is the atomic number?

A

The number of electrons is equal to the number if protons which is equal to the number of neutrons.

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17
Q

What is the isotopes of an atom?

A

The number of electrons is equal to the number of protons but not the numbers of neutrons.

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18
Q

How does atomic number help us to design the periodic table?

A

The arrangement of atoms from left to right according to increasing number of electrons (atomic number) and vertically according to the number of electrons on the outermost shell of the atom.

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19
Q

What is a full shell?

A

A nobel gas.

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20
Q

What is the outermost shell?

A

The valence shell.

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21
Q

What does each layer/shell represent?

A

A row in the periodic table.

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22
Q

What does each electron that you add represent?

A

A vertical column in the periodic table. Ex: 2 electrons on the 4th shell= calcium which is in the second vertical shell.

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23
Q

What is the hydrogen (H) shell pattern?

A

1

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24
Q

What is the lithium (Li) shell pattern?

A

2,1

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25
Q

What is the sodium (Na) shell pattern?

A

2,8,1

26
Q

What is the potassium (K) shell pattern?

A

2,8,8,1

27
Q

What is the rubidium (Rb) shell pattern?

A

2,8,18,8,1

28
Q

What is the cesium (Cs) shell pattern?

A

2,8,18,18,8,1

29
Q

What is the francium (Fr) shell pattern?

A

2,8,18,32,18,8,1

30
Q

What is the beryllium (Be) shell pattern?

A

2,2

31
Q

What is the magnesium (Mg) shell pattern?

A

2,8,8

32
Q

What is the calcium (Ca) shell pattern?

A

2,8,8,2

33
Q

What is the strontium (Sr) shell pattern?

A

2,8,18,8,2

34
Q

What is the barium (Ba) shell pattern?

A

2,8,18,18,8,2

35
Q

What is the radium (Ra) shell pattern?

A

2,8,18,32,18,8,2

36
Q

What is the fluorine (F) shell pattern?

A

2,7

37
Q

What is the chlorine (Cl) shell pattern?

A

2,8,7

38
Q

What is the bromine (Br) shell pattern?

A

2,8,18,7

39
Q

What is the iodine (I) shell pattern?

A

2,8,18,18,7

40
Q

What are ions?

A

They are atoms that have lost or gained electrons.

41
Q

How do we know the charge on an ion?

A

Ions are formed when the atoms loose electrons are negatively charged.

42
Q

What are positively charged ions called?

A

Cations.

43
Q

What are negatively charged ions called?

A

Anions.

44
Q

How do we form CaCl2?

A

Ca has 2e- on the outermost shell, to get to 8e- it would have to add 6e- which is harder then losing 2e- so we get Ca2+ as the charge.
Cl has 7e- on the outermost shell so we add 1e- to get 8e- and we get Cl- and its Cl2 so 2Cl-
ca2+ + 2Cl- = CaCl2

45
Q

How do we balance Fe + Cl2 = FeCl2?

A

2Fe + 3Cl2 = 2FeCl3

46
Q

What are the 3 main types of binary (ionic) compounds?

A

Type 1: Metal+non metal
Type 2: Metal+ non metal
Type 3: Non metal+ non metal

47
Q

What are type 1 compounds?

A

Type 1 metals that exhibit only one type of valence. They can only form one type of ion.

48
Q

How do we name type 1 compounds?

A 
Name the metal first then name the non metal by taking the first part of its name and adding -ide. 
Ex: NaF = Sodium Fluoride
      CaF2 = Calcium Fluoride
      AlF3 = Aluminum Fluoride
      KI = Potassium Iodide 
      Ba+Cl = BaCl2 = Barium Chloride
      Sr + Br = SrBr2 = Strontium Boride
49
Q

What are type 2 binary ionic compounds?

A

Type 2 metals are metals that exhibit more then one type of valence. They can form more then one type of ion and most of them are transition metals.

50
Q

How do we name type 2 compounds?

A

Name the metal first, then name the non metal, then use roman numerals in brackets after the name to indicate the charge on the metal.
Ex: Fe = Fe2+ = Iron (II) = Ferrous = Fecl2 = Iron (II) Chloride = Ferrous Chloride

51
Q

How do we name type 2 compounds (old name)?

A

Name the metal then add the ending “ous” for the lower charged ion and “ic” for the higher charged ion. Then name the non metal.
Ex: Fe = Fe2+ = Ferrous Chloride
Fe = Fe3+ = Ferric Chloride

52
Q

How do we name type 3 compounds?

A

Treat first element in compound as metal. Name it first. Then treat second element as non metal. Then use frefixes to indicate the total numbernof atoms of each element in the compund.
Ex: monocarbon monooxide

53
Q

What is the rule for polyatomic ions?

A

Ate: more oxygen
Ite: lower oxygen concentrate

54
Q

How do we name bromine (Br) ?

A 
Br0- = Hyperbromite
Br02- = Bromite
Br03- = Bromate
Br04- = Perbromate

Pay extra close attention to Chromate = Cr042- and Dichromate = Cr2072-

55
Q

What are oxyacids?

A

Oxyacids are acids containing oxygen. They are mostly formed by adding hydrogen to the polyatomic anion.

56
Q

How are oxyacids named?

A

They are named by using the name of the first non metal in the oxyanion plus the ending -ic (for the higher oxygen containing oxyanion) or -ous ( for the lower oxygen containing oxyanion) then adding acid.
Ex: H2SO4 = ate = Sulfuric acid
H2SO3 = ite = Sulfurous acid

57
Q

What are non-oxyacids?

A

Acids that do not contain oxygen.

58
Q

How do we name non-oxyacids?

A

Prefix by word hydro, then add the “root” name of the non metal, then add the ending -ic then the word acid.
Ex: HCl = Hydrochloric acid
HBr = Hydrobromic acid

59
Q

What are bases?

A

A base if a compound containing OH- ion. Compound contains positively charged ions and OH.

60
Q

How do we name bases?

A

Name the metal the add the word hydroxide.
Ex: Sodium hydroxide
Aluminum hydroxide

61
Q

What are salts?

A

Salts are compounds containing a positively charged ion and a negatively charged ion combined together.

62
Q

How do we name salts?

A

Name them by naming the positive ion and then name the negative ion.
Ex: (NH4)2SO3 = Ammonium Sulfite
MgC2042- = Magnesium Oxalate

Sec 5 Chemistry Dawson College (2 decks)

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