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(1) General chemistry > Unit 2: chemical composition > Flashcards

Unit 2: chemical composition Flashcards

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1
Q

What are the 7 diatomic elements?
*Have no fear of ice cold beer

A
  • Hydrogen (H)
  • Nitrogen (N)
  • Oxygen (O)
  • Fluorine (F)
  • Chlorine (Cl)
  • Bromine (Br)
  • Iodine (I)
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1
Q

What is matter?

A

Anything that has mass and occupies volume.

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2
Q

What’s matter that has constant propreties and composition?

A

A pure substance

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3
Q

What’s matter that doesn’t have constant properities and composition?
What are the 2 types?

A

A mixture!
Can either be heterogeneous or homogeneous.

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4
Q

What’s an element?

A
  • Fundamental unit of matter made up of only one type of atom
  • Cannot be chemically changed into a simpler substance without changing it’s properties.
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5
Q

All naturally occurring elements are stable and non-radioactive?

A

False!
Exemple, uranium and francium are unstable!

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6
Q

How many elements in periodic table?

A

118 elements and 90 naturally occuring, the rest are synthetic.
Each element is represented by a name and a symbol.

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7
Q

What’s atomic number, atomic weight and mass number?

A
  • Atomic number, Z, is the number of protons in the atom’s nucleus.
  • Atomic weight, mass, is the weighted average of all atoms of an element.
  • Mass number, A, is the sum of protons and neutrons in atoms nucleus.
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8
Q

Families/groups?

A
  • 18 vertical volumns
  • Numbered 1 through 18
  • All elements in a family have the same number of valence electron and similar chemical propreties
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9
Q

Periods?

A
  • 7 horizontal rows
  • All elements in a period have the same number of shells (couches électroniques)
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10
Q

3 categories in the periodic table?

A

1- Main group of elements (colomns 1A-2A and columns 3A-8A)
2- Transition metals (B groups 3-12)
3- Inner transition metals (lanthanides and actinides)

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11
Q

Common groups - Metals?

A
  • Left side of the zigzag line (except for hydrogen)
  • Solid at room temperature, conduct heat and electricity, lustrous, malleable and ductile
  • Loses electrons and for cations in chemical reactions
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12
Q

Common groups - nonmetals?

A
  • Right side of the zigzag line
  • 11 are gases, 5 are solid and 1 liquid (Br) at room temperature
  • Poor conductors of heat and electricity, non-lustrous and brittle.
  • Gain electrons and form anions in chemical reactions.
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13
Q

Common groups - semimetals (metalloids)?

A
  • Along the zigzag line; B, Si, Ge, As, Se, Sb and Te
  • Metal properties: solid, shiny, conduct heat and conduct electricity at high temperatures
  • Non metallic propreties: brittle
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14
Q

Groupe 1A: Alkali metals?

A
  • Soft silvery metals
  • Typically found as a compound because of reactivity (and stored in oil)
  • Low melting points and boiling points
  • Low densities
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15
Q

Groupe 2A: Alkaline Earth metals?

A
  • Relatively soft and reactive
  • Not found naturally in pure state
  • Lustrous, shiny silver metals
  • Relatively low melting and boiling points
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16
Q

Groupe 7A: Halogens

A
  • Liquids and gases at room temperature
  • Low melting and boiling points
  • Not found naturally in their pure state - reactive
  • Brittle when solide
  • Poor conductors
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17
Q

Group 8A: Noble gases

A
  • Odourless, colourless and nonreactive
  • Gases at room temperature
  • Low boiling points
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18
Q

Evolution of model of the atom?

A

1803: Dalton
1897: Thomson
1912: Rutherford
1913: Bohr
1930+: Schrodinger

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19
Q

What are the 3 particules in an atom?

A

1- Electrons (e-)
- Electron cloud outside of the nucleus
- Negatively charged
- Not very massive

2- Protons (p+)
- In the nucleus
- Positive charge
- Massive

3- Neutrons (n0)
- In the nucleus
- No charge
- Massive

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20
Q

What’s an isotope?

A
  • Atoms with identical atomic numbers (number of protons), but different mass numbers (different number of neutrons).
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21
Q

What’s the octet rule?

A

Fill valence shell to attain a noble gas electron configuration and become stable.

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22
Q

2 types chemical bonds?

A

Covalent bonds - sharing electrons
Ionic bonds - transfer of electrons

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23
Q

Covalent bond?

A
  • Sharing electrons between nonmetals
  • Prefixes indicate number of atoms of each element (mono, di, tri, tetra, penta, hexa, hepta, octa, nona and deca)
  • How to name? First element = full name. Second element = first part of it’s name and adding -ide + prefixes if needed. (Ex: Dinitrogen trioxide)
  • Do not use the prefix mono when there is only one atom of the first element (ex: carbon monoxide)
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24
Q

Specific names for some compounds?

A

H20 = water
H2O2 = hydrogen peroxide
NH3 = ammonia

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25
Q

Ionic compounds?

A
  • Transfer of electrons from one atom to another atom.
  • Results in a force of attraction between charged particules.
  • Metal and nonmetals.
  • Don’t add prefix with ionic bonds and read from left to read!
  • Ionic coumpouds are neutral, so net charge is always zero.
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26
Q

What is an ion?

A

An atom or a group of atoms that has a positive or negative charge.

27
Q

Cation?

A
  • Lost an electron
  • Positively charged
  • Ex: Metals
28
Q

Anion?

A
  • Gained an electron
  • Negatively charged particule
  • Ex: nonmetals
29
Q

Type 1 ionic compound?

A
  • Type 1: metal can only form 1 type of cation
  • Cation is placed first and anion is placed second with the ending changing in -ide.
30
Q

Type 2 ionic compound?

A
  • Type 2: metal can form 2 or more cations of different charges
  • Charge is specified by using Roman numerals (in parentheses) following the name of the metal.
  • Name the anion like usual.
  • Ex: Fe2O3 = Iron (3) oxide
31
Q

Elements with multiple charges?

A
  • Cr2+/Cr3+
  • Mn2+/Mn3+
  • Fe2+/Fe3+
  • Co2+/Co3+
  • Cu+/Cu2+
  • Hg2*2+/Hg2+
  • Sn2+/Sn4+
  • Pb2+/Pb4+
32
Q

Polyatomic ions?

A

Charged species containing 2 or more atoms bound together.
- Have a charge ex: +/2+/-…
- Ex: NH4+, NO3-

33
Q

Atomic mass unit?

A
  • AMU is used because the mass of an atom is very small.
  • Relative to the mass of 1 atom of carbon-12
  • Avergae mass of all the isotopes of an element
34
Q

The Mole?

A
  • Established to count atoms because atoms are so small
  • Equals the number of carbon atoms in exactly 12.011 grams of carbon
  • 1 mole = 6.022 x 10*23 atoms (avogadro’s number)
35
Q

Molar mass?

A

Molar mass of any substance is the mass (in grams) of 1 mole of that substance.

36
Q

Molecular weight?

A

Sum of individual atomic molar masses of the atoms that make up a compound.

37
Q

Name of Hg2*2+?

A

Mercury

38
Q

Name of NH4*+?

A

Ammonium

39
Q

Name of NO2*-?

A

Nitrite

40
Q

Name of NO3*-?

A

Nitrate

41
Q

Name of SO3*2-?

A

Sulfite

42
Q

Name of SO4*-2?

A

Sulfate

43
Q

Name of OH*-?

A

Hydroxide

44
Q

Name of CN-?

A

Cyanide

45
Q

Name of PO4*3-?

A

Phosphate

46
Q

Name of HPO4*3-?

A

Hydrogen phosphate

47
Q

Name of H2PO4*-?

A

Dihydrogen phosphate

48
Q

SCN-?

A

Thiyocyante

49
Q

CO3*-2?

A

Carbonate

50
Q

HCO3-?

A

Hydrogen carbonate

51
Q

ClO-?

A

Hypochlorite

52
Q

ClO2-

A

Chlorite

53
Q

ClO3-

A

Chlorate

54
Q

ClO4-

A

Perchlorate

55
Q

C2H3O2-

A

Acetate

56
Q

MnO4?

A

Permanganate

57
Q

Cr2O7*2-?

A

Dichromate

58
Q

CrO4*2-?

A

Chromate

59
Q

O2*-2?

A

Peroxide

60
Q

C2O4*2-?

A

Oxalate

61
Q

S2O3*-2?

A

Thiosulfate

62
Q

Molar mass?

A

Number of grams in 1 mol of an element

63
Q

Mass number?

A

Number of protons and neutrons in an element

64
Q

Atomic weight?

A

Weighted average of the isotopic masses of an element’s naturally occuring

65
Q

Atomic mass?

A

Mass of a specific atom

66
Q

Atomic number?

A

Quantity determined by the number of protons in an element

(1) General chemistry (9 decks)

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