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Yr 8 Science > Y8 AT2 - Half Yearly Exam (Chemistry) > Flashcards

Y8 AT2 - Half Yearly Exam (Chemistry) Flashcards

Flashcards for Year 8 Half Yearly Exam, Topics = Working Scientifically, Chemistry (90 cards)

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1
Q

Who proposed the atomic model stating that all matter consists of tiny particles called atoms?

A

John Dalton

Dalton’s model asserted that atoms of the same element are alike and atoms of different elements vary in size and mass.

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2
Q

What did John Dalton’s atomic model claim about atoms?

A

Atoms are indivisible and can be combined in simple whole number ratios

This claim was later disproven as atoms can be subdivided into protons, neutrons, and electrons.

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3
Q

What is the main idea of JJ Thomson’s Plum Pudding model?

A

Atoms contain negatively charged electrons embedded in a positively charged sphere

This model was later disproved by Rutherford’s gold foil experiment.

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4
Q

What was the key finding from Rutherford’s gold foil experiment?

A

The existence of a small, positively charged nucleus in atoms

Most alpha particles passed through the foil, indicating atoms are mostly empty space.

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5
Q

What did Niels Bohr propose about electron orbits?

A

Electrons orbit the nucleus at different levels in fixed paths

Electrons can move between levels by gaining or losing energy.

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6
Q

What did Erwin Schrödinger contribute to atomic theory?

A

Described electron locations as regions where electrons are most likely to be found

His model replaced the idea of fixed orbits with probabilistic electron clouds.

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7
Q

List the three subatomic particles that make up an atom.

A
  • Protons
  • Neutrons
  • Electrons
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8
Q

What is the structure at the center of an atom called?

A

Nucleus

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9
Q

Identify the location and charge of protons in an atom.

A

Located in the nucleus, charge: +1

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10
Q

Identify the location and charge of neutrons in an atom.

A

Located in the nucleus, charge: Neutral

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11
Q

Identify the location and charge of electrons in an atom.

A

Located in the electron cloud, charge: -1

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12
Q

What does atomic number represent?

A

The number of protons in an atom’s nucleus

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13
Q

What is the periodic law?

A

Elements with similar properties recur at regular intervals when arranged by atomic number

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14
Q

What trend is observed in atomic radii as you move down a group in the periodic table?

A

Atomic radii increase

More electron shells are added, making atoms larger.

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15
Q

What trend is observed in atomic radii as you move across a period?

A

Atomic radii decrease

Increasing nuclear charge pulls electrons closer to the nucleus.

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16
Q

Where are metals located on the periodic table?

A

Left and center of the periodic table

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17
Q

Where are non-metals located on the periodic table?

A

Right side of the periodic table

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18
Q

Define semimetals.

A

Elements with properties of both metals and non-metals

Located along the zig-zag line between metals and non-metals.

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19
Q

What are alkali metals?

A

Highly reactive metals found in Group 1

Examples include lithium and sodium.

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20
Q

What are noble gases?

A

Non-reactive gases found in Group 18

Examples include helium and neon.

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21
Q

What is the chemical formula for water?

A

H2O

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22
Q

What is the chemical formula for carbon dioxide?

A

CO2

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23
Q

What is the chemical formula for methane?

A

CH4

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24
Q

Fill in the blank: The modern periodic table is arranged by increasing _______.

A

atomic number

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25
What are the main categories of elements in the periodic table?
* Metals * Non-metals * Metalloids
26
What is an isotope?
Atoms of the same element with different numbers of neutrons
27
What are the general physical properties of metals?
* State at room temperature: Solid * Electrical conductivity * Thermal conductivity * Malleability * Ductility * Lustre
28
What is a compound?
A substance formed when two or more elements are chemically bonded together
29
What is the difference between a molecule and a compound?
A molecule is two or more atoms bonded together; a compound is a molecule that contains at least two different elements.
30
What does the periodic table organize elements based on?
Atomic number and recurring chemical properties.
31
What happens to atomic radii across a period?
Atomic radii decrease.
32
What happens to atomic radii down a group?
Atomic radii increase.
33
How are elements classified in the periodic table?
Metals, non-metals, and metalloids.
34
Name four groups found in the periodic table.
* Alkali metals * Alkaline earth metals * Halogens * Noble gases
35
What are the two main categories of properties of elements?
Physical Properties and Chemical Properties.
36
What are physical properties?
Properties that can be observed or measured without changing the identity of the substance.
37
Give three examples of physical properties.
* Colour * Melting point * Boiling point
38
What defines chemical properties?
How an element reacts with other substances, leading to a change in chemical composition.
39
List examples of chemical properties.
* Flammability * Reactivity * Acidity
40
What is the state of metals at room temperature?
Mostly solid (except mercury).
41
What is the electrical conductivity of metals?
High conductivity.
42
What is the malleability of metals?
Can be hammered or rolled into sheets.
43
What is the ductility of metals?
Can be stretched into wires.
44
What is the lustre of metals?
Shiny or metallic appearance.
45
What are the general physical properties of non-metals?
* State at room temperature: Solid, liquid, or gas * Electrical conductivity: Poor conductors * Thermal conductivity: Low conductivity * Malleability: Brittle * Ductility: Brittle * Lustre: Dull appearance
46
What is a metal lattice?
A regular arrangement of metal atoms held together by metallic bonds.
47
How does the atomic structure relate to the reactivity of Group 1 elements?
Fewer valence electrons lead to easier electron loss and high reactivity.
48
What are alkali metals known for?
Highly reactive, especially with water.
49
What characterizes alkaline earth metals?
Less reactive than Group 1 but still react with water.
50
What defines halogens?
Highly reactive non-metals, especially with alkali metals.
51
What are noble gases known for?
Inert gases that do not readily form compounds.
52
What is the octet rule?
Atoms like to have a full octet (eight electrons) in their valence shell.
53
What are covalent bonds?
Bonds formed when two non-metal elements share electrons.
54
What is an ionic bond?
A bond formed through the attraction between positively and negatively charged ions.
55
What is a molecule?
A small number of atoms bonded together.
56
Define a diatomic molecule.
Molecules with two atoms.
57
What is a polyatomic molecule?
Molecules with more than two atoms.
58
What is the maximum number of electrons in the first shell?
2 electrons.
59
What is the maximum number of electrons in the second shell?
8 electrons.
60
What is the maximum number of electrons in the third shell?
18 electrons (or 8 for the first 20 elements).
61
How do you determine what ion will form from an atom?
By calculating the total number of electrons and determining stability.
62
What happens when an atom loses electrons?
It becomes a positive ion.
63
What happens when an atom gains electrons?
It becomes a negative ion.
64
What is the formula for water?
H₂O.
65
What is the formula for sodium chloride?
NaCl.
66
Fill in the blank: The outer shell of an atom is called the _______.
valence shell.
67
What ion is formed when Beryllium loses 2 electrons?
Be²⁺ ## Footnote Beryllium has an atomic number of 4 and loses 2 electrons to achieve stability.
68
What ion does Oxygen form when it gains 2 electrons?
O²⁻ ## Footnote Oxygen has an atomic number of 8 and requires 2 additional electrons to complete its octet.
69
What ion is formed when Aluminium loses 3 electrons?
Al³⁺ ## Footnote Aluminium has an atomic number of 13 and loses 3 electrons to achieve stability.
70
What type of bond occurs between metal atoms?
Metallic Bond ## Footnote Metallic bonds involve a lattice structure where electrons are delocalized.
71
What is formed in a covalent bond?
Small molecule or covalent network ## Footnote Covalent bonds involve the sharing of outer electrons.
72
What type of bond occurs between a metal and a non-metal?
Ionic Bond ## Footnote Ionic bonds are formed through electrostatic attraction between oppositely charged ions.
73
What are the characteristics of gas substances at room temperature?
Low melting & boiling points ## Footnote Examples include Hydrogen, Nitrogen, Oxygen, Fluorine, and Chlorine.
74
What is the melting point of Sodium Chloride?
801 °C ## Footnote The boiling point of Sodium Chloride is 1465 °C.
75
What type of bonds lead to high melting and boiling points?
Metallic and ionic bonds ## Footnote These bonds are strong, resulting in high melting and boiling points.
76
Why do covalent molecules have low melting and boiling points?
Only weak forces between molecules need to be broken ## Footnote Strong covalent bonds within the molecules remain intact.
77
What is the role of weak intermolecular forces in ice?
They hold the molecules together as a solid ## Footnote When melting, heat energy breaks these weak forces.
78
What do Lewis Dot Diagrams represent?
Valence (outer shell) electrons as dots ## Footnote Dots are positioned around the atom to show electron pairs.
79
What is the first step in creating a Lewis Dot Diagram?
Add up total valence electrons ## Footnote This is essential for accurately representing the molecule.
80
In a Lewis Dot Diagram, what is done after drawing the symmetrical structure?
Place lone electron pairs around outer atoms ## Footnote Hydrogen is an exception and is completed with a single bond.
81
How many valence electrons are there in water (H₂O)?
8 valence electrons ## Footnote This is calculated as 2 from Hydrogen and 6 from Oxygen.
82
What is the total number of valence electrons in carbon dioxide (CO₂)?
16 valence electrons ## Footnote This includes 4 from Carbon and 6 from each of the 2 Oxygen atoms.
83
Fill in the blank: Covalent network substances have _______ melting and boiling points.
very high ## Footnote This is due to the very strong bonds in their structure.
84
What happens to the bonds in a lattice when it melts?
The bonds between atoms in the lattice need to break ## Footnote The stronger the bond, the more heat energy required.
85
What type of intermolecular force do small covalent molecules have?
Weak intermolecular forces ## Footnote These forces lead to lower melting points.
86
What are the formulas of: - Water - Carbon Dioxide - Hydrochloric Acid - Carbon Monoxide
- H2O - CO2 - HCl - CO
87
What are the formulas of: - Glucose - Methane - Sodium Chloride - Ammonia - Nitric Acid - Sulfuric Acid
- C6H12O6 - CH4 - NaCl - NH3 - HNO3 - H2SO4
88
What are the three types of atomic bonds?
Covalent, Ionic, Metallic
89
What is the electron configuration for Calcium?
(2, 8, 8, 1)
90
What are three properties that can be used for non-metals & metals?
- state at room temperature - electrical conductivity - thermal conductivity - malleability - ductility - lustre

Yr 8 Science (2 decks)

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