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Chemistry Exam GR 11 > Unit 1: Matter, Chemical Trends, and Bonding > Flashcards

Unit 1: Matter, Chemical Trends, and Bonding Flashcards

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1
Q

What are the 3 ways of representing an element?

A

Example: Sodium

(23 is the mass number and 11 is the atomic number)

1) 23

Na

11

2) Na- 23
3) Sodium - 23

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2
Q

What do “A” and “Z” represent?

A

A= Mass Number

Z= Atomic Number

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3
Q

When given that Potassium has 19 protons and 20 neutrons how would you determine A and Z?

A

Z= 19 (Atomic Number/ Number of Protons)

A= Z + N = 19 + 20 = 39 (Atomic Mass)

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4
Q

Isotope

A

An element which has the same number of protons in all its other forms but a different number of neutrons. They have the same chemical properties but their physical appearance differs. ( Same Z; Different A)

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5
Q

What is Heavy Water? What is it’s chemical formula?

A

Water that contains hydrogen in the form of deuterium.

D2O

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6
Q

Mass Spectrometer

A

A device used to determine the atomic mass and relative abundance of each isotope present in an element.

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7
Q

amu

A

Atomic Mass Unit

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8
Q

Radio Isotopes

A

Isotopes and are unstable and decay emitting radiation as their nucleus changes.

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9
Q

What are the 3 types of radiation, their speed, their penetration distance, and an example of an effective barrier?

A

1) Alpha Slow, A few cm, and a sheet of paper
2) Beta Fast, A few m, 1-2mm of metal
3) Gamma Very fast, unlimited, 1m of lead or concrete

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10
Q

Alpha Particles

A

A particle composed of 2 protons, 2 neutrons and equivalent to a helium nucleus with a charge of 2+.

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11
Q

Beta Particles

A

A high energy electron with a charge of 1-.

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12
Q

What is the concept of Half- Life?

A

The time taken for half of a radio active atoms to decay in a radioactive substance.

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13
Q

What is the concept of Carbon- 14 Dating?

A

The measurement of a ratio of Carbon- 14 to Carbon- 12 to determine how long and organism has been dead. They compare the normal ratio of a living organisms to a dead one to find the time that has elapsed.

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14
Q

What happens when the amount of Carbon-14 in a sample becomes very small?

A

The Carbon-14 dating method becomes less reliable.

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15
Q

What other method can be used to date non-living materials? What is it’s half life?

A

Potassium-40 is used to date objects too old to be effectively dated by the carbon-14 method. It’s half life is 1.3 X 109 years.

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16
Q

What happens to the alkali metals as their atomic number increases?

A

The elements are more reactive.

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17
Q

What is Atomic Radius? List the 2 Facts you need to know about what it does and why it does them.

A

One half the distance between the nuclei of 2 atoms of the same element.

1) Decreases from left to right across each period on the periodic table. -The atomic number increase by 1 for each element- therefore increasing by 1 proton as we move right. - The attraction between the nucleus and valence electron increases pulling the electron in tighter. (Radius smaller)
2) Increases from top to bottom down each group on the periodic table - The number of valences increases as we go down a group - More valences means more of a shield to attract the valence electrons to the nucleus.

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18
Q

What is Ionic Radius? List the 2 facts you need to know about Cations and Anions in terms of their atomic radius.

A

Cations: 1) Ionic Radius becomes smaller across a period/ row - As a cation looses electrons the ionic radius decreases - The attraction of the electrons to the nucleus increases across a period/ row - The nucleus would be able to pull the electrons closer to the nucleus

Anions: 1) Ionic Radius Increases across a period/ row - When gaining an electron the repulsion among electrons increases while nuclear charge remains the same - Nucleus will not be able to pull the electrons as close to the nucleus - They fill the outer shell therefore radius becomes larger

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19
Q

What is Ionization Energy?

A

The amount of energy required to remove an electron from an atom or ion in the gaseous state.

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20
Q

What is the Difference between First Ionization Energy and Second Ionization Energy?

A

First Ionization Energy: The amount of energy required to remove the most weakly held electron from a neutral atom

Second Ionization Energy: The amount of energy required to remove a second electron from the gaseous positive ion

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21
Q

What is Multiple Ionization Energies?

A

After the first electron is removed the valence shell hets a little closer to the nucleus (Increse in effective nuclear charge) It will now take more energy to remove the 2nd electron.

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22
Q

What is Electron Affinity? What is its example equation and its trend?

A

The energy change that occurs when an electron is accepted by a neutral atom in the gaseous state (Energy will be released).

X(g) + e-→x-(g) + Energy

Cl (g) + e- →Cl-(g) + 349 kj/mol

Electron Affinity increases across a period (row) and decreases down a group (column)

23
Q

What is Electronegativity? What is it’s trend?

A

The ability of an atom (When bonded) to attract electrons. The attraction between the valence electrons and the nucleus decreses as the distance between them increases.

Electronegativity increasesacross a period (row) and decreses down a group (coloumn)

24
Q

What is Electrical Conductivity? How does it differ in Ionic and Molecular compounds?

A

The ability of a material to allow electricity to flow through it. You can use this to determine which kind of compound a substance is.

Ionic Compounds: Form solutions that conduct electricity

Molecular Compounds: Form solutions that don’t conduct electricty

25
Q

Electrolytes vs Non-electrolytes

A

Electrolytes: Substances that form solutions that conduct electricity

Non-Electrolytes: Substances that form solutions that do not conduct electricity

26
Q

What are the 3 properties of Ionic Compounds?

A

1) Solids at SATP
2) High Melting and Boiling Points
3) Electrolytes

27
Q

Which groups on the periodic table tend to gain and lose electrons?

A

Gain: 15, 16, 17

Lose: 1, 2 ,3

28
Q

What are the electrons in a covalent bond doing?

A

They’re being shared

29
Q

Lone pair

A

A pair of valence electrons not involved in the bonding.

30
Q

Bonding Capacity

A

The number of covalent bonds (Shared electron pairs) that an atom can form.

31
Q

Electronegativity

A

The ability of an element to attract one electron.

32
Q

What will happen if one element has a higher electronegativity than the other element it’s bonded to?

A

The electrons will spend more time with the more electronegative element.

33
Q

Polar Covalent Bond

A

A covalent bond formed between atoms with significantly different electronegativities.

34
Q

The greater distance in electronegativity…

A

The more polar and ionic the bond becomes.

35
Q

What is the range to decide whether a bond is

a) Non-Polar
b) Polar Covalent
c) Ionic

A

a) Non-Polar: Difference 0.0 - 0.4
b) Polar Covalent: Anything greater than 0.4 but less than 1.7
c) Ionic: Anything greater than 1.7

36
Q

Ionic Bond

A

A intramolecular force that involves an electron transfer resulting in the formation of cations and anions which attract eachother.

37
Q

Polar Covalent Bond

A

An intramolecular force that involves unequal sharing of pairs of electrons between 2 elements. They can involve paris of 1, 2 or 3 (1 being weak and 3 being strong).

38
Q

Non-Polar Covalent Bond

A

A intramolecular force that involves equal sharing of pairs of electrons. The bonds can have pairs of 1, 2 or 3. (1 being the weakest and 3 being the strongest)

39
Q

Intramolecular force

A

The attractive force within a compound.

40
Q

Intermolecular Force

A

The attractive force between molecules.

41
Q

Are Intramolecular or Intermolecular Forces Stronger?

A

Intramolecular.

42
Q

van der Waals Forces

A

Weak intermolecular attractions.

43
Q

What are the 3 van der Waals Forces?

A

1) Dipole- Dipole
2) London Dispersion Force
3) Hydrogen Bonding

44
Q

Which of the 3 van der Waals Forces is the strongest?

A

Hydrogen Bonding.

45
Q

Hydrogen Bonds

A

A relatively strong dipole-dipole force between a positive hydrogen atom of one molecule and a highly electronrgative atom (F, O or N) in another molecule.

46
Q

Cohesion

A

Water molecules are attracted to one another. they’re made up of (-) oxygen and (+) hydrogen atoms. The (+) hydrogens are attracted to the (-) oxygens of the other molecules and vice versa. This attractive force is what gives water its cohesive properties.

47
Q

Surface Tension

A

The cohesion of water molecules at the surface of a body of water. This forms a “film” or “skin” which strength can be refused by some substances.

48
Q

Adhesion

A

Forces of attraction between a liquid and another surface

49
Q

What is the Abrieviation for rembering the Acids? What does each bolded word and letter stand for?

A

NICK the CAMEL had a CLAM for SUPPER in PHOENIX

Each bolded word represents one of the oxyacids.

The constants= # of oxygens in the formula

The vowels= # of hydrogens in the formula

50
Q

What are the 5 main oxyacids?

A

1) Nitric Acid
2) Carbonic Acid
3) Chloric Acid
4) Sulphuric Acid
5) Phosphoric Acid

51
Q

What happens when you remove the H’s from each word in the acids abbriviation. What does their charge represent?

A

It creates a “ate” polyatomic ion

Example: Nitric Acid (HNO3) makes Nitrate (NO3)

The charge represents the number of hydrogens in the acid

52
Q

What are the 3 ways we can alter Ions in relation to acids?

A

1) Adding an oxygen

From “ate” → Per_____ate

Example: Chlorate (ClO3) → Perchlorate (ClO4)

2) Removing an oxygen

From “ate” → “ite”

Example: Chlorate (ClO3​) → Chlorite (ClO2)

3) Removing 2 oxygens

From “ate” → Hypo_____ite

Example: Chlorate (ClO3​) → Hypochlorate (ClO)

53
Q

What are Hydrates? What happens to them when they’re heated?

A

A compound that contains water as a part of its ionic crystal strcuture.

When heated, it will decompose to an ionic compound and water vapour when heated.

54
Q

Gamma Rays

A

Electromagnetic Wavelengths and the most dangerous type of radiation.

Chemistry Exam GR 11 (6 decks)

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