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Chem Quiz/Test Flashcards > Chem Quiz - pg 1-10 > Flashcards

Chem Quiz - pg 1-10 Flashcards

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1
Q

What is the Atomic Theory?

A

Atomic theory is the scientific theory that matter is composed of particles called atoms

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2
Q

Dalton’s Atomic Theory

A
  • all matter is composed of tiny, individual particles called atoms
  • atoms of an elemnet have identical properties
  • atoms of different elements have different properties
  • atoms of two or more elements can combine in constant ration to form a new substance
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3
Q

J.J. Thompson’s Atomic Theory

A

Raisin Bun
- discovery of electrons
- raisun bun or plum pudding model
- atom is sphere which is positive, with negative electrons embedded in it like raisins in a bun
- most of the mass is associated with the psotive charge

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4
Q

Ernest Rutherford’s Atomic Theory

A

Nucleus
- atoms have a nucleus which is positive and has most of the mass
- most of the atom is empty space, occupied by the moving negatively charged atoms
- propsed the existence of protons

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5
Q

Neils Bohr’s Atomic Theory

A

Planetary Model
- electrons move in circular orbits around the nucleus
- cannot exist between orbits

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6
Q

James Chadwick’s Atomic Theory

A

Neutrons
- showed that the nucleus mus contain heavy neutral particle to account for all of the atom’s mass (neutrons)

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7
Q

Schrodinger/de Broglie’s Atomic Theory

A

Quantum Model
- Quantum Mechanical model
- electrons have distinct energy levels
- exact location of electrons are not defined, but the probable reaction in a region of space can be predicted

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8
Q

What is a Proton?

A
  • positive charge subatomic particle
  • found in nucleus
  • determines the type of element
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9
Q

What is a Neutron?

A
  • neutral charge subatomic particle
  • found in nucleus
  • used to hold nucleus together
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10
Q

What is an Electron?

A
  • smallest subatomic particle
  • negative charge
  • found in “cloud” region
  • arranged in energy levels
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11
Q

What is Atomic Mass?

A
  • AMU is the mass of a proton or neutron = 1.7 x 10 to the power of -24g
  • net charge for all atoms is 0
  • e- = #p+ in a neutral atom
  • mass number is the sum of protons and neutrons (rounded to nearest whole number)
  • used to find the number neutrons
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12
Q

What is an Isotope?

A
  • atoms that have same number of protons but a different number of neutrons
  • atomic mass on the periodic table is an average mass based on the % abundances of all naturally occuring isotopes of the element
  • provide atomic mass in the name
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13
Q

The Periodic Table

A
  • Metals
  • Non Metals
  • Metalloids along stair case
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14
Q

What is the Atomic Number?

A
  • number of protons in one atom of an element
  • increases from left to right and top to bottom
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15
Q

What are the properties of Metals?

A
  • good conductors
  • strong
  • malleable
  • ductile
  • high lustre
  • are found on left side of staircase
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16
Q

What are the properties of Non-Metals?

A
  • poor conductors
  • non lustrous
  • weak
  • non ductile
  • non malleable
  • opposite properties of metals
  • found on right side of staircase
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17
Q

What are the properties of Metalloids?

A
  • shows properties of both metals and non metals
  • found along the stair case
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18
Q

How many groups are there in the Periodic Table?

A
  • 18 vertical groups called families
  • labelling system: Roman Numeral and letters or ordinary numbers
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19
Q

What is Group 1 (IA)?

A

Alkali Metals (very reactive)

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20
Q

What is Group 2 (IIA)?

A

Alkaline Earth Metals (less reactive)

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21
Q

What is Group 17 (VIIA)?

A

Halogens (reactive non metals)

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22
Q

What is Group 18 (VIIIA)?

A

Inert or Noble Gases (unreactive)

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23
Q

What is the Lanthanide Series (IA)?

A

Rare Earth (57-71)

24
Q

What is Group 3-12 (B Series)

A

Transition Metals

25
Q

Elements in each group share _______?

A

Similar chemical properties although intensity changes

26
Q

Reactivity _______ for Metals and _______ for Non Metals

A

Down group for Metals and Up Group for Non Metals

27
Q

The Group Number indicates ____?

A

How many electrons are in the outer most energy level

28
Q

What are Periods?

A
  • horizantal rows
  • show a trend in reactivity which changes left to right
  • each time you move to a new period you start the trend over
29
Q

What is an EELD?

A

Energy Electon Level Diagram

Level 4 - max 8e-
Level 3 - max 8e-
Level 2 - max 8e-
Level 1 - max 2e-

  • energy levels- shows number of e- in each level (# of levels = period)
30
Q

What are Ions?

A

Ions are atoms or groups that have a net charge
- number of protons and electrons are not equal
- most atoms try to achieve the electron configuration of a nobel gas

31
Q

What does Isoelectronic mean?

A

means having the same number of electrons as another atom or ion

eg) fluorine gains an electron to be isoelectronic with neon

32
Q

What are Cations?

A
  • Positively charged ions
  • lost electrons to obtain a stable electron configuration (full valence level)
  • charge on a metal ion is the same as the group number for groups 1,2,3,13,14
  • metals form Cations
33
Q

What are Anions?

A
  • negatively charged ions
  • gained electrons to obtain a stable electron configuration (full valence level)
  • charge on a non-metal is 18-group #
34
Q

How do you write a EELD for atoms?

A

P+
E-
N
Level 4 - 2e-
Level 3 - 8e-
Level 2 - 8e-
Level 1 - 2e-
Nucleus (Proton and Neutrons)
Element Symbol

35
Q

How do you write a EELD for ions?

A

Level 4 - 2e- (charge on top)
Level 3 - 8e-
Level 2- 8e-
Level 1- 2e-
Nucleus (Proton and Neutron)
Element Symbol with Charge

*make sure to bracket all of the EELD

36
Q

What is the EELD formula for Ions?

A

P = atomic number
E = # of protons - charge
N = atomic mass - atomic number

eg) sodium
P = 11
E = 11 - (+1) = 10
N = 12

37
Q

Atoms have _______ and Ions have ________

A
  • Atoms have same e- and p+, no charge
  • Ions have either negative or positive charge
38
Q

Metallic elements exist as _____

A

Single atoms, monatomic

39
Q

Chemical is the _____ followed by the ______ at room temperature

A

Symbol, State

40
Q

Non Metals do not exist as _______ and are called _______

A

Single Atoms, Molecular Elements

41
Q

Molecular compounds are formed when?

A

2 or more non metals bond together

42
Q

Molecular compounds are bonded by?

A

Covalent bonds which is the force of attraction between atoms that are sharing electrons

43
Q

Properties of Molecular Compounds

A
  • Do not conduct electricity when dissolved in water
  • dissolve in water to form a neutral molecular solution or an acidic solution
  • solid, liquid or gas at room temperature
44
Q

How do you name Molecular Compounds?

A
  • give the atom name for the first element (with prefix if there is more than one)
  • give the name for the second element, add ide ending and include prefix

*if first element is hydrogen, no prefix it is an acid

eg) CO(g) Carbon Monoxide

45
Q

What are the prefixes?

A

1 - Mono
2 - Di
3 - Tri
4 - Tetra
5 - Penta
6 - Hexa
7 - Septa
8 - Octa
9 - Nona
10 - Deca

46
Q

How do you write Molecular Formulas?

A

Write each symbol followed by the subscript (from prefix)

47
Q

What is Ammonia?

A

NH3

48
Q

What is Water?

A

H2O

49
Q

What is Methane?

A

CH4

50
Q

What is Methanol?

A

CH3OH

51
Q

What is Ethane?

A

C2H6

52
Q

What is Ethanol?

A

C2H5OH

53
Q

What is Glucose?

A

C6H12O6

54
Q

What is Sucrose?

A

C12H22O11

55
Q

What is Ozone?

A

O3

56
Q

What is Hydrogen Peroxide

A

H2O2

Chem Quiz/Test Flashcards (2 decks)

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