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Physical Science > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

What does Hund’s Rule state?

A

there is no p, d or f orbitals before each orbital in that orbital has at least 1 electron

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2
Q

What does Paul’s Exclusion Principal state

A

there is a maximum of 2 electrons in each orbital provided they have an opposite spine

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3
Q

What branches does matter break into?

A
  1. Pure substances
    1.1 Elements
    1.2 Compounds
  2. Mixtures
    2.1Homogeneous
    2.2 Heterogeneous
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4
Q

What different type of elements are found in nature?

A

Metals, Non-Metals, Metalloids

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5
Q

Define heterogeneous mixture?

A

A mixture with a non-uniform composition and all the components can be distinguished

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6
Q

Define Homogeneous mixture.

A

a mixture with a uniform composition and all the components are in the same state. (that will remain constant for a period of time).

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7
Q

Define element.

A

pure substances composed of any type of particle

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8
Q

define Compound.

A

pure substances composed of 2 or more different elements.

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9
Q

Define Freezing Point.

A

the temperature at which a liquid completely changes into a solid when heat is removed.

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10
Q

define Melting point

A

the temperature at which a solid completely changes into a liquid when heat is added.

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11
Q

define boiling point.

A

the temperature at which the vapor pressure is equal to the surrounding atmospheric pressure in a liquid

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12
Q

Define the term Evaporation.

A

the process whereby a liquid changes to a vapor at any temperature below boiling point.

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13
Q

define the term Condensation.

A

the process where a gas or a vapor changes to a liquid by cooling or increasing the pressure.

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14
Q

What does the Law of Conservation of Mass state

A

the total mass of particles before a state change and the total mass after a state change remains constant ( in a closed container)

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15
Q

define the term defusion.

A

the movement of the particles of a substance in between the particles of a second substance from a high to a low concentration

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16
Q

What does Brownian Motion state

A

the random motion of microscopic particles is suspension in a liquid or gas. It is caused by collisions between these particles and the molecules of a liquid or gas.

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17
Q

How do we identify chemical formulae.

A

we use the ions of elements , then cross multiply them as well as make sure that hey are in their simplest form.

(Always make sure that you balance the equation)

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18
Q

Define the term stock notation.

A

tells us the valency of the transition metals

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19
Q

Define the term atomic mass

A

Number of protons in the nucleus and also indicates the elements position on the periodic table

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20
Q

Define the term Mass

A

the number of protons and neutrons in the nucleus

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21
Q

Define the term Orbital

A

a region of space in which the probability of finding an electron is high

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22
Q

What are the 7 diatomic elements found in nature?

A
  1. Iodine
  2. Chlorine
  3. Bromine
  4. Florine
  5. Oxygen
  6. Nitrogen
  7. Hydrogen
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23
Q

Define the term Ion

A

a small charged particle which is a result of a neutral atom either losing or gaining electrons

24
Q

What is a Negative Ion referred to as?

A

Anion

25
Q

What is Positive Ion referred to as?

A

Cation

26
Q

Define the term Atom

A

a neutral particle

27
Q

Define the term Isotope.

A

Atoms that have the same number of protons but different number of neutrons.

OR…

Atoms that have the same atomic number but different mass numbers.

28
Q

If an isotope only has the same has a singular particle what is it referred to as?

A

A Protium

29
Q

If an isotope has a an equal amount of protons and neutrons what is it referred to as?

A

a Deterium

30
Q

what can the group numbers on the periodic table tells us?

A
  1. they can tell us how many valence electrons are in an atom
  2. they can tell us the valency of an atom
31
Q

define the term Core electrons

A

these are electrons in the inner energy level

31
Q

Define the term Valence Electron.

A

these are the electrons in the outermost energy level

32
Q

What is Group 1 on the periodic table known as?

A

Alkali metals

33
Q

What is Group 2 known as on the periodic table?

A

Alkaline Earth metals

34
Q

What is the middle section of the periodic table known as?

A

Transition metals

35
Q

What is group 7 on the periodic table known as?

A

Halogens

36
Q

What is group 8 on the periodic table known as?

A

Nobel Gases

37
Q

Define the term Ionization energy.

A

the energy needed per mol to remove an electron/ electrons from an atom in the gaseous state.

38
Q

What are the 2 types of ionization energy?

A

First ionization energy and second ionization energy

39
Q

What is the first ionization energy?

A

The energy needed per mol to remove the first electron from an atom in a gaseous state

40
Q

What is the second ionization energy?

A

the energy needed per mol to remove the second electron from an atom in the gaseous state.

41
Q

Is it easier or more difficult to remove an atom if the ionization energy is higher?

A

More difficult

42
Q

What is the unit for ionization energy?

A

KJ. 1/mol

43
Q

Define the term electron affinity.

A

the amount of energy released when a neutral atom accepts an additional electron to form a negative ion

44
Q

What does the Law of constant composition state?

A

it ensures that mass cannot be created or destroyed. It requires the same number of atoms of each element to be on either side of the equation

45
Q

Define the term Mol.

A

the quantity of matter that has the same number of particles (atoms, molecules or ions) as there are atoms in 12 grams of Carbon-12

46
Q

What 2 types of changes can you get?

A

A physical and chemical change

47
Q

Name the 2 types of chemical changes.

A

synthesis and decomposition

48
Q

If a molecule is ionic, what are its particles called?

A

Formula units

49
Q

Define the term chemical bond.

A

a mutual attraction between 2 atoms resulting from the simultaneous attraction between their nuclei and the outer electrons.

50
Q

Name the 3 types of chemical bonds.

A
  1. Covalent bond (non-metal + non-metal)
  2. Ionic bond (non-metal + metal)
  3. Metallic bond (metal + metal)
51
Q

Define the term covalent bond.

A

the sharing of electrons between atoms to form molecules.

52
Q

Define the term Ionic bond.

A

the transfer of electrons to form cations and anions that attract each other to form a formula unit.

53
Q

Define the term metallic bond.

A

the bond between positive ions and delocalized valence electrons in metals.

54
Q

In a compound if one atom is electro positive and another is electron negative what is the bond called?

A

the bond is polar

55
Q

In a compound if both atoms are either electronegative or electropositive what is the bond called?

A

the bond is non-polar

Physical Science (2 decks)

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