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Science 2016 > Glossary Terms Chapter 4- Chemistry > Flashcards

Glossary Terms Chapter 4- Chemistry Flashcards

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1
Q

Atomic Number

A

Number of protons in an atom

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2
Q

Atoms

A

The particles that make up all materials; the smallest part of an element that can take part in a chemical reaction

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3
Q

Electron configuration

A

Arrangements of electrons in electron shells

i.e. 2, 8, 8, 2

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4
Q

Electron shells

A

Also known as energy levels, the regions surrounding the nucleus where electrons may be found.

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5
Q

Element

A

A substance with one type of atom only, with the same atomic number; 118 are known to exist.

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6
Q

Energy levels

A

Also known as electron shells, the regions surrounding the nucleus where electrons may be found.

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7
Q

Ground state

A

The lowest energy arrangement of an atom’s electron in energy levels (shells).

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8
Q

Indirect evidence

A

Evidence that does not involve direct observation.

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9
Q

Nucleus

A

Heavy core at the centre of an atom, made of protons and neutrons.

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10
Q

Compound

A
  • 2 or more different elements chemically combined.

eg. water= H2O (H and O are 2 different elements)

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11
Q

Molecule

A
  • 2 or more atoms chemically combined
  • Can be the same or different
  • Discrete groupings of atoms covalently bonded together
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12
Q

Atomic Mass number

A
  • The larger number in the element (excluding hydrogen which is 1 for both numbers)
  • protons and neutrons combined
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13
Q

Atomic number

A
  • The smaller number in the element
  • The number of protons
  • The number of electrons
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14
Q

How do you calculate the number of neutrons?

A

By subtracting the atomic number from the atomic mass number.

eg. 2 In Helium, 4-2=2, so there are 2 neutrons
He
4

    3           In Lithium, 7-3=4, so there are 4 neutrons
    Li
     7
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15
Q

How are elements arranged in columns in the periodic table?

A

Elements are in columns/groups, depending on how many electrons are in their outer shell. (from left to right- 1 in outer shell= first column etc.)
- Also goes across in rows/periods by an increase of 1 for each.

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16
Q

How many electrons does N-3 have?

A

+3 electrons

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17
Q

Define an Ion

A
  • Also known as ‘charged atoms’

- An atom that can gain or lose electrons. Electrons are transferred from one atom to another.

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18
Q

What charge is an ion that loses electrons?

A

Positive Charge

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19
Q

What charge is an ion that gains electrons?

A

Negative Charge

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20
Q

Actinides

A

A special block of metallic elements with atomic numbers 90-103

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21
Q

Groups

A

Vertical columns of the periodic table; group number is equal to the number of electrons in the outer shell of atoms of elements in that group.

22
Q

Lanthanides

A

A special block of metallic elements with atomic numbers 58-71

23
Q

Periodic Table

A

A list of all the known elements, arranged horizontally in order of increasing atomic number and vertically according to the number of electrons in the outer shell.

24
Q

Periods

A

Horizontal rows of the periodic table; period number of an element is equal to the number of electron shells

25
Q

Transition elements

A

A special block of metallic elements covering elements from groups 3-12

26
Q

Bonds

A

Links that join atoms together

27
Q

Covalent bonding

A
  • Between non-metals
  • The sharing of electrons between atoms

Has two types:
- Giant Covalent Network
Diamond (lattice of carbons)

  • Discreet Covalent Molecules
    Water (have low melting and boiling points and is an insulator)
  • Now have neutral charge and no attraction between molecules
28
Q

Inert gases

A

Also known as noble gases, group 18 elements known for their stability and lack of reactivity

29
Q

Ionic bonding

A
  • Between a metal and non-metal
  • Attraction of positive and negative ions formed from the transfer of electrons from metallic to non-metallic atoms
  • This is called Electrostatic Attraction and forms lattices.

**** A lattice is a regular arrangement of something. Ionic compounds form a lattice. (large temperatures will turn ionic compounds into a liquid).

30
Q

List the properties of ionic compounds

A
  • Solids at room temperature
  • High melting and boiling points (energy required)
  • Brittle / shatter easily
  • Poor conductors (in solid state)
    (good conductors when dissolved in water or molten- such as NaCl2- salt water)
31
Q

Lattices

A

A regular arrangement of particles. Ionic compounds form lattices (large temperatures turn ionic compounds into liquid).

In ionic lattices, particles are ions
In solid molecular lattices, particles are molecules
In diamond and graphite, particles are atoms

32
Q

Metallic Bonding

A

A mutual attraction between a lattice of positive metal ions and a sea of delocalised, outer shell electrons. The ion sea enables the structure to become malleable, ductile and thermal/electrical conductors.

33
Q

What are the properties of metals?

A
  • High melting and boiling points (except mercury)
  • Good thermal and electrical conductors
  • Malleable
  • Ductile
  • Sonourous (ringing sound when you strike it)
  • Lustre (colourful lustre: coins)
  • Solid at room temperature (except mercury= liquid)
34
Q

Monatomic

A

Atoms existing on their own, without bonding with others

35
Q

Noble gases

A
  • Also known as inert gases, group 18 elements known for their stability (lack of reactivity)
  • Are monatomic and do not bond
  • Extremely stable (full outer electron shells)
  • Single atom that rarely reacts with other atoms.
36
Q

How do chemical bonds form?

A

The sharing or transfer of electrons makes a chemical bond form.

37
Q

Alkali metals

A

Group 1 elements

38
Q

Alkaline earths

A

Group 2 elements

39
Q

Allotropes

A

Forms of the same element that have different molecular structures and therefore different properties

40
Q

What are the three allotropes of carbon?

A

Graphite, amorphous carbon / charcoal and diamond

41
Q

Halogens

A

Group 17 elements

42
Q

Organic

A

Compound that is or was part of a living thing; contains carbon

43
Q

Organic molecules

A

Molecules that have a backbone of carbon

44
Q

What are the factors which affect the rate of a reaction?

A

Reactants of a chemical reaction must collide with enough energy and in the correct orientation.
If this is increased, the reaction rate is faster.

Factors affecting rate of a reaction:

  • Temperature (more energy and particles move quicker)
  • Agitation / shake or stir it (mixes together / faster movement
  • Pressure and concentration (an increase in particles has a larger likely-hood of colliding)
  • Particle size (larger surface area / powder reacts faster)
  • Catalyst (aligns chemicals in correct orientation, increasing collisions and rate)
45
Q

Electrons in the outer-most shell have the ……… energy

A

highest

46
Q

Why does the # of protons = #of electrons?

A

The # of proton and electrons are equal because atoms are always electrically neutral

47
Q

The first electron shell has the …………. attraction to the nucleus.

A

strongest

48
Q

What determines the element an atom belongs to?

A

Its # of protons

49
Q

How many of the 118 elements are synthetic / man-made?

A

26

50
Q

What is the heaviest element?

A

Uranium is the heaviest element

  • Its extreme size makes uranium unstable and highly radioactive
  • When these nuclei break apart, massive amounts of energy are released, evident in the 1958 atomic bomb test.
51
Q

What are elements’ names based from?

A
  • The first letter
  • Two ‘logical’ letters
  • Temporary (Ununoctium / Uuo)
  • Original Greek or Latin name
    (Iron / Fe / Ferrum, Copper / Cu / Cuprum, Lead / Pb / Plumbum)

Science 2016 (5 decks)

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