Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Science Gr 10 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

What are some characteristics of metals?

A
  • lustrous
  • malleable
  • ductile
  • conductors of heat and electricity
  • Do not corrode
  • Usually solid at room temperature
  • high density
  • high melting and boiling points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are some characteristics of non-metals?

A
  • non-lustrous
  • brittle
  • poor conductors
  • Typically solid or gas
  • generally lower melting and boiling points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are some characteristics of metalloids?

A
  • intermediate between metals and non-metals
  • all solid at room temperature
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How are you meant to draw a Bohr Rutherford Diagram?

A
  • P: Protons (Atomic Number)
    E: Electrons (Atomic Number)
    N: Neutrons (Atomic Mass - Atomic Number)
  • 2 electrons on the first shell
  • 8 electrons on the next shell
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Physical Properties:

A
  • colour
  • size
  • shape
  • solubility
  • hardness
  • malleability
  • conductivity
  • Melting and boiling points
  • density
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Chemical Properties:

A
  • flammability
  • toxicity
  • acidity
  • reactivity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the meaning of something exothermic?

A

Something that produces heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is a precipitate?

A

The formation of a solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the difference between a chemical and physical property?

A

Physical: A property that can be determined without changing the substance’s chemical identity

Chemical: A property that can be determined only by changing the substance’s chemical structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does 2n^2 represent?

A

The number of electrons a shell could accommodate.
N represents the valence shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the difference between naming covalent and ionic compounds?

A

Covalent:
- use prefixes for both atoms (except for mono on the first one)
- change the suffix of second element to ide

Ionic:
- use NO prefixes
- change the end of second element to ide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a polyatomic ion?

A

An ion composed of more than one atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the polarity chart?

A

POLAR: 0-0.4
NON-POLAR: 0.5-1.6
IONIC: 1.7 and up

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

The name of a cation is the same as the name of the element.

Yet, what occurs with the name of an anion?

A

The ending of an anion is changed to ide

EX: Fluorine becomes Fluoride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Are metals more likely to become cations or anions? Why?

A

Cations (positive) as it is easier for them to lose electrons to have full valence shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How many valence electrons do metals and non-metals have?

A

Metals: 1-3
Non-metals: 5-7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the trend that exists down a group and across a period with ionic charges?

A

Down a group: ionic charge remains the same

Across a period: charges increase by 1 until 3, the increase by 1 from -3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

When an atom forms an ion, it becomes an isoelectronic to a noble gas. What does this mean?

A

An isoelectronic means that the atom has the same number of electrons as a noble gas

EX: Na loses one electron, giving it 10 electrons like Ne

F gains one electron, giving it 10 like Ne

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Practice using Lewis Dot diagrams to show bonding between various elements

19
Q

What is group 1 called and some of its properties?

A

Alkali Metals - soft and highly reactive

20
Q

What is group 2 called and some of its properties?

A

Alkaline Earth Metals - light, reactive metals

21
Q

What is group 17 called and some of its properties?

A

Halogens - highly reactive

22
Q

What is group 18 called and some of its properties?

A

Noble gases - most stable, rarely react with other elements, gases

23
Q

Practice finding the average atomic mass of isotopes

24
Practice finding the abundance of isotopes
25
What is an isotope?
An isotope is an element with the same number of protons but a different number of neutrons. Therefore, it is a version of an elementwith a different atomic mass Most elements have two or more naturally occurring isotopes, and the different isotopes are found in different abundance amounts of a given isotope that exists in nature, expressed as a percentage)
26
What is an atom's ionization energy?
The amount of energy an atom requires to remove an electron from itself The higher the ionization energy, the more difficult it is remove an electron
27
What is the radius of an atom?
The distance from the centre of an atom to the approximate boundary of their electron cloud
28
Explain the trend of the atomic radius on the periodic table
Down a group: INCREASES More shells Across a period: DECREASES Same number of shells, but the force of attraction between the nucleus and electrons increases, causing the electrons to move inward, shrinking the size of the atom
29
Explain the trend of ionization energy
Down a group: DECREASES With an increasing number of shells, the nucleus has a weaker ability to attract the electrons to the centre Across a period: INCREASES Across a period, the number of shells remains the same, but the number of protons increases. Hence, they attract the electrons to the center with greater strength
30
Explain the electron affinity trend
Down a group: DECREASES As you move down a group, electrons are further from the nucleus, causing it to be harder to attract electrons from the nucleus Across a period: INCREASES Across a period, the number of valence electrons increases. Hence, the atom is more likely to want to gain enough electrons to have a full valence shell
31
What is electron affinity?
A measure of how much an atom wants to gain an electron Also The energy change when an electron is added to an atom
32
What is electronegativity?
A measure of the ability of an atom to attract electrons to itself
33
Explain the trend with electronegativity
Down a group: DECREASES With an increasing amount of electrons and valence shells around the nucleus, it is harder for the nucleus to attract more electrons Across a period: INCREASES As you move across a period, the number of valence electrons increases, causing the atom to gain the remaining electrons required for it be stable (full valence shell)
34
Why can't 2 non-metals or two metals form an ionic compound?
Because non-metals are more likely to gain electrons and have full valence shells. Hence, if they become ions, they will both be anions and will, therefore, not be attracted to one another.
35
What is the difference between a covalent and ionic bond?
Covalent: - Only between non-metals - Atoms share electrons rather than giving them to one another - They share the electrons to have full valence shells (the electrons orbit) Ionic: Atoms give one another electrons, causing them to be opposite ions that attract to one another (electrostatic attraction
36
What is a double covalent bond? What is a triple covalent bond?
Double: When the atoms share two sets/pairs of electrons Triple: When atoms share three sets/pairs of electrons
37
What is the difference between electron affinity and electro negativity?
Affinity: - how much an atom wants to attract an electron Negativity: - the ability of an atom to attract electrons towards itself
38
When do you use the negative delta sign, and when do you use the positive sign?
The negative sign goes for the atom with the HIGHER electro-negativity
39
Why doesn't atomic number have a full correlation with the radius?
As you move across the period, the atomic number increases, but the radius decreases. However, as you go down a group, atomic number increases, and so does the radius
40
Why does electron affinity increase across a period? Up a group?
Electron affinity increases across a group as atoms are closer to having full valence shells and, therefore, wish the most to have another electron to stabilize them. Also, up a group, electron affinity increases because there are less valence shells, making the force of the nucleus stronger.
41
Why does electro negativity increase across a period and up a group?
Because more to the right of the period, atoms have more protons and a stronger ability to attract electrons. Also, up a group, as there are fewer valence shells, allowing the force of the nucleus to be strong enough to attract more electrons.
42
What do the numbers in an ionic compound and a molecular compound represent?
Ionic: the ratio that the given ions are present in Molecular: the number of atoms of each element present (not in a ratio)
43
Which element receives the positive delta sign? Which receives the negative delta sign?
Negative: goes to the element with the greater electronegativity Positive: goes to the element with the smallest electronegativity NOTE: Electronegativity is the ability of an atom to attract other electrons towards itself
44
When do you use the delta sign, and why?
Only in polar bonds because polar bonds have unequal electron distribution. Therefore, the positive and negative delta signs demonstrate the unequal distribution
45

Science Gr 10 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions