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Chem Grade 11 > Exam Review > Flashcards

Exam Review Flashcards

1
Q

What is matter?

A

It’s anything that has mass and takes up space.

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2
Q

What is an atom?

A

It’s the smallest unit of matter that has the properties of an element.

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3
Q

What is a compound?

A

A substance formed when two or more chemical elements are chemically bonded together.

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4
Q

What is a chemical property?

A

A change of a material’s properties that happen during or after a chemical reaction (basically any quality that can be seen only by changing a substance’s chemical identity)

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5
Q

What is a physical property?

A

Physical properties can be observed or measured without changing the composition of matter.

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6
Q

What is a physical change?

A

It is changes affecting the form of a chemical substance, but not its chemical composition.

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7
Q

What is an electron?

A

The smallest of the particles that make up an atom and they have a negative charge -1

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8
Q

What is a proton?

A

It’s a subatomic particle found in an atom and has a positive charge +1 (opposite of an electron)

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9
Q

What is a neutron?

A

It’s a subatomic particle found in the nucleus of atoms and is neutral (zero charge)

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10
Q

What is a molecule?

A

The smallest particle in a chemical element or compound that has the chemical properties.

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11
Q

What is a mixture?

A

A material made up of two or more different substances which are mixed but are not combined chemically.

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12
Q

What is ionization energy?

A

The amount of energy required to remove the most loosely bound electron (the valence electron) to form a cation.

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13
Q

What is a solution?

A

A homogeneous mixture composed of two or more substances

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14
Q

What is a concentration?

A

The number of molecules or ions in a given volume of a substance, expressed as mol/L (molarity).

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15
Q

What is a solute?

A

A substance dissolved in another substance, known as a solvent.

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16
Q

What is a solvent?

A

A substance that dissolves a solute resulting in a solution

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17
Q

What is a homogeneous mixture?

A

A mixture which has uniform composition and properties throughout. ie. oooooooo

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18
Q

What is a heterogeneous mixture?

A

A mixture in which the components can be seen ie. oooo0o0oo

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19
Q

What is a qualitative chemical analysis?

A

The identification of elements or grouping of elements present in a sample

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20
Q

What is a quantitative chemical analysis?

A

the determination of the absolute or relative abundance (usually expressed as a concentration) of one, a bunch or all substance(s) in a sample.

21
Q

What is isoelectronic?

A

Refers to two atoms, ions or molecules that have the same electronic structure and same number of valence electrons.

22
Q

What is the activity series?

A

A chart of metals listed in order of declining relative reactivity. The top metals are more reactive than the metals on the bottom.

23
Q

What is the Law of Conservation of Mass?

A

This law states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations. Mass of product in chemical reaction = mass of reactants.

24
Q

What is the Law of Definite Proportions?

A

(Proust’s law) States that a chemical compound always contains its component elements in fixed ratio (by mass)

25
Q

What is the Law of Constant Composition?

A

States that all samples of a chemical compound have the same elemental composition by mass

26
Q

What is an atomic mass unit?

A

Unit of mass used to express atomic and molecular weights.

27
Q

What is atomic mass?

A

Mass of an atom of a chemical element. The mass number is the total number of protons and neutrons combined

28
Q

What is the molecular mass?

A

The mass of a molecule.

29
Q

What is molar mass?

A

For ie. mmH2O=18.01 (16+2(1.01). It’s just the masses added up.

30
Q

What is an ion?

A

An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

31
Q

What is a cation?

A

A positively charged ion

32
Q

What is an anion?

A

A negatively charged ion

33
Q

What is an isotope?

A

The number of protons in an atom’s nucleus. For example, an atom with 6 protons must be carbon

34
Q

What is electron affinity?

A

The amount of energy released or spent when an electron is added to a neutral atom or molecule

35
Q

What is a pure substance?

A

Homogeneous substance that has consistent properties throughout the sample.

36
Q

What is electronegativity?

A

Tendency of an atom to attract a bonding pair of electrons.

37
Q

What are valance electrons?

A

The outside electrons are the most easily lost.

38
Q

What is an ionic bond?

A

The complete transfer of valence electron(s) between a metal and non-metal

39
Q

What is a covalent bond?

A

The sharing of electron pairs between two non metals.

40
Q

What is a non polar covalent bond?

A

A type of chemical bond where two atoms share a pair of electrons with each other.

41
Q

What is a polar covalent bond?

A

A type of chemical bond where a pair of electrons is unequally shared between two atoms.

42
Q

What is effective nuclear charge?

A

The net positive charge experienced by an electron in a multi-electron atom.

43
Q

What is the periodic law?

A

Properties of the elements are periodic functions of their atomic numbers. Also called Mendeleev’s law.

44
Q

What is a period? A group?

A

Period is across the table. Group is down the table (which is a chemical family).

45
Q

Group names on the periodic.

A
  1. Alkali metals
  2. Alkali earth metals
    3-12. Transition metals
    13-16. No approved names
  3. Halogens
  4. Nobel gases
46
Q

Contribution each scientist made on the structure of the atom:
Dalton, Thompson, Rutherford and Bohr.

A

Dalton- Proposed that all matter is composed of very small things which he called atoms.

Thompson- Proposed the plum pudding model of the atom that had no nucleus and is composed of + and - charged particles.

Rutherford- An atom is mostly empty space, with electrons orbiting a fixed, positively charged nucleus in set, predictable paths.

Bohr- Depicted the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus

47
Q

Periodic trends: Increase or decrease?

  • atomic radius
  • 1st ionization energy
  • electronegativity
A

Atomic radius
Across period= decrease
Down a group= increase

1st ionization energy
Across period= increase
Down a group= decrease

Electronegativity
Across period= increase
Down a group= decrease

48
Q

What group of elements has the lowest electron affinity? Why?

A

Metals. Because metals lose electrons to become balanced rather than gain

Chem Grade 11 (4 decks)

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