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Chemisty > Chemistry > Flashcards

Chemistry Flashcards

1
Q

What are atoms?

A

The basic units of matter made up of protons, neutrons, and electrons.

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2
Q

What is the nucleus of an atom?

A

The dense center of an atom containing protons and neutrons.

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3
Q

What are electrons and where are they found?

A

Negatively charged particles found in shells (energy levels) around the nucleus.

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4
Q

What defines an element?

A

A substance made of only one type of atom, with a specific number of protons.

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5
Q

How are elements represented?

A

By chemical symbols, e.g., H for hydrogen and O for oxygen.

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6
Q

What is a compound?

A

A substance formed when two or more elements chemically bond.

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7
Q

How do compounds differ from mixtures?

A

Compounds have fixed ratios and are chemically bonded, while mixtures are physically combined.

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8
Q

What is a reactant in a chemical reaction?

A

A substance present at the start of a reaction.

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9
Q

What is the product in a chemical reaction?

A

The substance formed after the reaction.

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10
Q

What was Dalton’s atomic theory?

A

All matter is made of indivisible atoms, which combine in fixed ratios.

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11
Q

What did J.J. Thomson discover?

A

The electron, leading to the plum pudding model of the atom.

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12
Q

What was Rutherford’s gold foil experiment?

A

It showed atoms have a dense, positive nucleus surrounded by empty space.

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13
Q

How did Bohr improve the atomic model?

A

He proposed electrons orbit the nucleus in fixed energy levels.

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14
Q

How did Mendeleev organize the periodic table?

A

By increasing atomic mass and grouping elements by similar properties.

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15
Q

What key change occurred in the modern periodic table?

A

It is organized by atomic number, not mass.

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16
Q

What are groups in the periodic table?

A

Vertical columns that contain elements with similar chemical properties.

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17
Q

What are periods?

A

Horizontal rows that show elements with the same number of electron shells.

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18
Q

What trend occurs across a period?

A

Atomic size decreases, and elements become less metallic.

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19
Q

What are properties of metals?

A

Conduct electricity, malleable, ductile, shiny, and high melting points.

20
Q

What are properties of non-metals?

A

Poor conductors, brittle, dull, and low melting points.

21
Q

Why are Group 1 metals so reactive?

A

They have one electron in their outer shell, which is easily lost.

22
Q

What happens when alkali metals react with water?

A

They produce hydrogen gas and an alkaline solution.

23
Q

How does reactivity change down Group 1?

A

Reactivity increases because the outer electron is farther from the nucleus.

24
Q

What are the states of halogens at room temperature?

A

Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

25
Q

What is displacement in halogens?

A

A more reactive halogen displaces a less reactive halogen from its compounds.

26
Q

How does reactivity change down Group 7?

A

Reactivity decreases as it is harder to attract electrons.

27
Q

Why are noble gases unreactive?

A

They have full outer electron shells.

28
Q

How do boiling points change down Group 0?

A

Boiling points increase due to stronger intermolecular forces.

29
Q

What is an ion?

A

An atom or group of atoms with a positive or negative charge.

30
Q

How do metals form ions?

A

By losing electrons to form positive ions (cations).

31
Q

How do non-metals form ions?

A

By gaining electrons to form negative ions (anions).

32
Q

What is ionic bonding?

A

The transfer of electrons between a metal and a non-metal.

33
Q

What holds ionic compounds together?

A

Strong electrostatic forces between oppositely charged ions.

34
Q

What are properties of ionic compounds?

A

High melting points, soluble in water, and conduct electricity when molten or dissolved.

35
Q

What is covalent bonding?

A

The sharing of electrons between two non-metals.

36
Q

What is a single covalent bond?

A

One pair of shared electrons.

37
Q

What are simple molecular substances?

A

Small molecules with strong covalent bonds but weak intermolecular forces.

38
Q

Why do simple molecular substances have low boiling points?

A

Weak intermolecular forces require little energy to overcome.

39
Q

What are examples of giant covalent structures?

A

Diamond, graphite, and silicon dioxide.

40
Q

Why is diamond hard?

A

Each carbon atom forms four strong covalent bonds.

41
Q

Why does graphite conduct electricity?

A

It has delocalized electrons between its layers.

42
Q

Why does reactivity increase down Group 1?

A

The outer electron is farther from the nucleus, making it easier to lose.

43
Q

Why does reactivity decrease down Group 7?

A

Attracting an extra electron becomes harder due to increased shielding.

44
Q

Why do noble gases have higher boiling points as you go down the group?

A

Larger atoms have stronger intermolecular forces.

45
Q

What is the significance of the periodic table’s organization?

A

It predicts element properties and reactions.

46
Q

How does atomic size change across a period?

A

It decreases due to increased nuclear charge pulling electrons closer.

47
Q

What are alloys and why are they useful?

A

Mixtures of metals to improve strength, corrosion resistance, or other properties.

Chemisty (4 decks)

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