Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Grade 10- Science > Chemistry > Flashcards

Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
Biology 101 flashcards
1
Q

Metals

A 
Metals make up the left side and the majority of elements on the periodic table.
Good conductors
Malleable- can become a wire
Ductile
Shiny- lustrous
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Non-metals

A

Poor conductors
Brittle when solid
Not ductile
Dull- not lustrous

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

Metalloids= between metals and non- metals

A

Solid at room temperature

Semi-conductors

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

Information in Periodic Tables

A

The smaller number on top is the atomic number which represents the number of protons in an atom.
The number of protons= the number of electrons
The one or two letter atomic symbol represents the name of the element
The largest number is the atomic mass→ the number of protons + neutrons added together
Protons and neutrons have a mass of one atomic unit.
Electrons have close to a mass of zero

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

Ernest Rutherford’s model of an atom

A

Gold foil experiment
The experiment showed that the majority of the mass of the atom is found in a small nucleus in the centre.
The nucleus is where positive protons and neutral neutrons are located.
He determined the rest of the atom was mostly empty with very small negatively charged electrons scattered around the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Bohr Rutherford Model

A

Neils Bohr started to work with Rutherford in 1911

Together, they modified Rutherford’s model to make it include electron orbitals.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The four Families in the Periodic Table

A

Alkali metals
Alkaline earth metals
The Halogens
The noble gases

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

Element

A

A substance that cannot be broken down into smaller parts

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

Compound/ molecule

A

a pure substance that can be broken into smaller parts.

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

When two or more atoms react to produce a new substance→

A

chemical bonds are formed

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

Chemical bonds involve electrons being

A

shared/ passed between two or more atoms

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

Ionic Bonds

A

Form when a metal gives up the valence electrons to a non-metal.
Commonly called salts
Form compounds with 2 or more ions
Ions: atoms with lost or gained electrons
Ions are written in square brackets with charge
Positively charged= cation
Negatively charged= anion

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

Properties of Ionic Compounds

A

Form crystals
Melt at high temperatures
Conduct electricity when dissolved in water
Hard + brittle
Chemical formulas represent formula unit of crystal.
Ex. NaCl

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

Covalent Bonds

A

Formed when two or more non- metals share electrons → forming a chemical bond
Form molecules instead of compounds
Ex. NH3

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

Properties of Covalent Bonds

A

Low melting and boiling points
Covalent molecules tend to be more flammable than ionic compounds
When dissolved in water, it does not conduct electricity
Some form crystals, but most are in other forms
Molecular formulas show the exact number of each atom in the molecule.

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

Nomenclature

A

a branch of taxonomy concerned with the application of scientific names to taxa, based on particular classification scheme and in accordance with agreed international rules + conventions.

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

IUPAC Nomenclature

A

a system of naming chemical compounds and for describing the science of chemistry. It is maintained by the International Union of Pure and Applied Chemistry.

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

Binary Compounds

A

contains two elements in a compound. May have multiple atoms of each element but can only have two elements.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Ionic Binary Compound

A

compound contains one metal and non-metal. Either element may have multiple atoms but there can only be two elements involved.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Ionic Binary Compounds: IUPAC Naming

A

Consists of two types of monatomic ions
The metal ion is always written first and retains the whole name
Non- metal is written second and the ending is changed to -ide.
Do not write 1s
If both elements have the same number, reduce to lowest terms.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Ionic Multivalent Binary Compounds

A

varied numbers of electrons in its valence shell. Occurs with elements that fall outside of representative elements.
Ex. transition metals
Means they can form compounds in various proportions.

22
Q

Multivalent Ionic Compounds

A

(ex. Copper and Oxygen): copper and oxygen could have two different formulas with two different properties.
CuO and Cu2O

23
Q

Ionic Multivalent Binary Compounds

A

same as ionic binary, but it indicates metals charge
List metal names first
After the metal name, indicate ion charge in brackets using roman numerals.
Add -ide to non-metal.

24
Q

Polyatomic Ions

A

Ions composed of more than one atom.
Entire molecule carries a charge
When determining the chemical formula of an ionic compound with a polyatomic ion, you treat polyatomic ion as a normal ion.

25
Q

Naming Ionic Polyatomic Compounds

A

Multivalent: metal (charge) polyatomic ion
Monovalent: metal polyatomic ion
Tertiary ionic compounds are comprised of a metal ion.
Write polyatomic the same way as monatomic ions.

26
Q

Oxyanions

A

Polyatomic ions that contain oxygen

27
Q

How to name oxyanions

A

ClO-hypochlorite ion→ hypochlorite
ClO2- chlorite ion→ chlorite
ClO3- chlorate ion→ chlorate
ClO4- perchlorate→ per-chorate

28
Q

Molecules

A

Made of covalent bonds, not ionic
Most compounds you find are molecular compounds
Sugar looks similar to salt, but they are very different

29
Q

Ionic vs. Molecular

A

If salt is dissolved in water, water would be conductive.
Ionic compounds conduct electricity.
Molecular compounds share electrons
Ionic compounds can only bond to non-metals in so many ways.
There are thousands more of molecular compounds than ionic compounds.

30
Q

Molecular Compounds

A

Made of two or more non-metals

Pair of shared electrons is called covalent bonds.

31
Q

Naming Electrons

A

Names of molecular compounds often contain prefixes which are used to count the number of atoms in the molecule.

32
Q

Naming Binary Molecule Compound: IUPAC

A

Write the name of the first element

If there is more than one atom, attach the Greek Prefix. Ex. CF4= carbon tetrafluoride

33
Q

Order of Elements: Binary Molecule Compound

A 
In ionic compounds, metal comes first.
In molecules, we use the hill system:
Carbon= first
Hydrogen= second if carbon is present if not, it is first
Everything else is alphabetical
34
Q

Chemical Reactions

A

Takes place when chemicals combine to create a new compound or molecule or when chemicals break apart to form new products.
Part reacting= reactant
New compounds are called products.
Reactions are written: reactant 1+ reactant 2→ product
Place states of matter with the elements
Skeleton equation: O2(g)+H2(g)–> H2O(l)

35
Q

Writing Chemical Equations

A

When writing, include states.

Aqueous means dissolved in a solution.

36
Q

Law of Conservation of Mass

A

Matter cannot be created or destroyed.
In a closed system, the mass of reactants will always equal the mass of the products.
Chemical reactions mean the number of atoms of a certain element in the reaction must be the same as the number of atoms in the product.

37
Q

Balancing Chemical Equations

A

Means we add coefficients to the front of products and reactants meaning we have that many of those chemicals.
Odd numbers usually don’t work.

38
Q

5 Main Types of Chemical Reactions

A 
Synthesis
Decomposition
Single Displacement
Double Displacement
Combustion
39
Q

Synthesis

A

A+B→ AB
A synthesis reaction: Two elements form a new product.
When given only two elements on the reactant side, determine product with crossover method.

40
Q

Decomposition

A

AB→ A+B
Occurs when a single compound or molecule breaks to smaller compounds.
When given only one compound or molecule, it will be individual elements.
HOFBrINCl → 2

41
Q

Single Displacement

A

A+BC→ AC+B
In single displacement, one element takes the place of another element.
Single displacement will only occur if the element being displaced is less reactive than the other.

42
Q

Double Displacement

A

AC+BD→ AD+BC
In a double displacement, two cations of different reactions exchange places to create new compounds.
Doubles occur if one of the following is true.
One product= water
One product= gas
One product= insoluble
Use the solubility test to determine if the product will form a precipitate.

43
Q

Combustion

A

Carbon reacts with oxygen to produce carbon dioxide, water and heat.

44
Q

Acids

A

compounds that produce hydrogen ions (H+) when dissolved in water. Ex. Hydrochloric Acid.
Each Chemical formula for an acid starts with hydrogen since it loses in water.

45
Q

Bases

A

compounds that produce hydroxide ions (OH) when dissolved in water. Ex. Sodium Hydroxide.
The bases each have hydroxide ions OH- since that is what it loses in water.

46
Q

Naming Binary Acids

A

Contain hydrogen and one non-metal. Ex. HBr
Steps
Write the root of the nonmetals name→ Bomine→ Brom.
Add hydro to the front→ Hydrobrom.
Add ic to the ending→ Hydrobromic

47
Q

Oxoacids + Naming them

A

Contain hydrogen, oxigen and one other element→ H2CO3
Naming Steps
Write the name of a polyatomic ion without the ate or ending→ Carbonate→ Carbon
If the polyatomic ended in ate, replae it with ic→ Carbonic acid
If the polyatomic ends in ite, replace it with ous→ Phosphorous acid

48
Q

Determining Formula From Name- Oxoacids

A

Determine if binary (starts with hydro) or oxoacid (does not start with hydro).
Identify the charge on the anion or polyatomic ion.
Use cross-over method to determine the formula with H+

49
Q

Naming Bases

A

*Same rules as naming compounds
Write the cation
Write the anion with ide.
*To find the formula for the base, use the crossover method.

50
Q

Acid/ Base Neutralization Reactions

A

When acids + bases are mixed, they neutralize each other.
When H+ ions react with OH- ions from the base, they form water.
Metal and Non-metals react and form ionic compounds
Neutralization Reaction: HABOH ? H2O+BA→ Acid+ Base? Water+ Ionic Compound.

Grade 10- Science (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions