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unit 1 & 2 flashcards > Unit 1 Chemistry > Flashcards

Unit 1 Chemistry Flashcards

(58 cards)

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1
Q

Describe the term “isotope” in relation to the number of protons, electrons and neutrons.

A

Isotopes are atoms of an element that have the same number of protons but different number of neutrons. Isotopes of the same element have the same electron configuration when neutrally charged.

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2
Q

Describe the chemical properties and physical properties of an isotope

A

Isotopes have the same chemical properties because they have the same number of electrons. Their physical properties, like mass and density, can be different due to the different number of neutrons.

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3
Q

What causes isotopes to have different physical property’s?

A

The varying number of neutrons causes isotopes to have different physical properties.

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4
Q

What charge does a neutral atom have?

A

A neutral charge.

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5
Q

What are the components of an atom, i.e. its subatomic particles?

A

Protons, nuetrons and electrons.

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6
Q

What is an ion?

A

An ion is an atom or group of atoms that has an electric charge.

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7
Q

What is the name of a positively charged ion?

A

Ions with a positive charge are called cations.

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8
Q

What is the name of a negatively charged ion?

A

Ions with a negative charge are called anions.

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9
Q

What is an isotope?

A

Atoms with the same number of protons but different numbers of neutrons.

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10
Q

What is the mass of a proton?

A

Protons in the nucleus each have a mass of 1.67 × 10–24 g.

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11
Q

What is the mass of an neutron?

A

(9.11 × 10–28 g)

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12
Q

What is aufbau’s principle?

A

electrons full atomic orbitals of the lowest available energy levels before occupying higher levels.

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13
Q

What is successive ionisation energy?

A

The energy required to remove the next electron.

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14
Q

What is condensed electron configuration also known as?

A

Noble gas notation.

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15
Q

How many orbitals does s have?

A

1 orbital (2e-)

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16
Q

How many orbitals does p have?

A

3 orbitals (6e-)

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17
Q

How many orbitals does d have?

A

5 orbitals (10e-)

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18
Q

What is the pauli exclusion principle?

A

No two electrons can occupy the same position or state.

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19
Q

What is Hund’s rule?

A

Every orbital in a subshell is singlely occupied before any orbital is doubly occupied.

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20
Q

What is the horizontal row called?

A

periods (1-7)

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21
Q

What is the veritcal row called?

A

groups (1-18)

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22
Q

What are some properties of metals?

A

(left) shiny solids, high melting points, conduct heat electricity.

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23
Q

What is Group 1 called?

A

Alkali.

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24
Q

What is group 2 called?

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A

Alkali earth metals.

25
What is group 17 called?
Halogens.
26
What is group 18 called?
Noble gas'.
27
What are some properties of non-metals?
low melting and boiling points, do not conduct heat and electricity, not shiny.
28
What are metalloids?
Where non-metals and metals overlap.
29
What is a nuclear charge?
Positive charge of nucleus creates electrostatic attraction with valence electrons (pulls them in).
30
What is the shielding effect?
Outer energy levels are 'shielded' from the pull of the nucleus by the inner energy levels. The greater the shielding effect, the lesser electrostatic attraction.
31
What is the atomic radius?
The size of an atom.
32
What is valency?
The atoms ability to form chemical bonds with another atom.
33
How many valance electrons are in ions that are smaller than the neutral atom?
4 valence electrons which will have a greater nuclear charge.
34
How many valence electrons for the ion to be greater than the neutral atom?
atoms with less than 4 valence electrons will from cations.
35
What is ionisation energy?
Amount of energy needed to remove an electron from a neutral gaseous atom.
36
What does low ionisation mean?
The easier it is to become an ion.
37
What is an example of low ionisation?
k(g) → k+(g) + e-
38
What does valency refer to?
atom’s ability to form chemical bonds with another atom
39
Describe the periodic tables valency trend.
Increases left-right, remains consistent down a group.
40
Describe atomic radious period table trend.
Increases right-left and down a group.
41
Describe ionic radius periodic table trend.
Increases as we move down a group.
42
Describe ionisation energy periodic table trend.
decrease down a group + increases left - right. (Shielding effect: valence electrons are furthur away from the nucelus).
43
What is Electronegativity?
the ability of an atom to attract the valence electrons of the adjacent atom. (attract atoms/electrons)
44
Describe electronegativity periodic table trend.
decreases down a group. increase left-right.
45
Define Metallic Character.
extent to which an element exhibits metallic properties. (high melting and boiling points, conductivity)
46
Describe Metallic Character periodic table trend.
Metallic character increases top right to bottom left, Non-metallic character increases from bottom left to top right.
47
What is an oxide?
Compounds that contain oxygen and another metal or non-metal element.
48
What makes up a basic oxide?
oxygen plus metal.
49
What properties does an atmospheric oxide have?
both acidic and basic properties.
50
What makes up an acidic oxide?
oxygen plus non-metal.
51
What are the 3 types of intermolecular bonds?
Ionic, Metallic and Covalent.
52
Define Intramolecular bonding .
bonding between atoms.
53
What happens to metals and non-metals in ionic bonding.
Metal atoms lose electrons, Non-metal atoms gain electrons.
54
What is ionic bonding?
the forces of electrostatic attraction holding ions together.
55
Name some physical properties of ionic bonds?
High melting and boiling point (solids at room tempurature), Does not conduct electricity or heat in a solid state, Giant lattice of repeating ions.
56
What is the Octet Rule?
the tendency to lose, gain or share electrons in order to achieve a full outer shell.
57
What is a Polyatomic ion?
ions which contain two or more atoms.
58
What is a monoatomic ion?
one atom with a charge.

unit 1 & 2 flashcards (5 decks)

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