Unit One Exam

Question 1

What is he unit for mass

Answer 1

Kilograms

Question 2

What is the unit for volume

Answer 2

Liters

Question 3

What is the unit for distance

Answer 3

Meters

Question 4

What are the subatomic particles that make up an atom

Answer 4

Protons, neutrons, and electrons

Question 5

Proton mass

Answer 5

1 amu

Question 6

Neutron mass

Answer 6

1 amu

Question 7

Electron mass

Answer 7

0 amu

Question 8

What happens if a proton moves from an atom

Answer 8

Element changes

Question 9

What happens if a neutron moves from an atom

Answer 9

Becomes isotope

Question 10

What happens if an electron moves from an atom

Answer 10

Becomes ion

Question 11

What force holds the nucleus of an atom together

Answer 11

Strong nuclear force

Question 12

What takes up the most space in an atom

Answer 12

Nothing, the majority of an atom is empty space

Question 13

What is the atomic number and what happens if the atomic number changes

Answer 13

The number of protons in the nucleus of an atom, and the element will change if the number of protons change

Question 14

Atomic mass

Answer 14

The average number of protons and neutrons inside the nucleus of an atom

Question 15

What are the scientific method steps

Answer 15

Question 
Background research 
Hypothesis 
Experiment 
Results
Conclusion 
Publish

Question 16

9. What is atomic mass?

Answer 16

The average number of protons and neutrons inside the nucleus of an atom

Question 17

10. What is mass number?

Answer 17

Mass number is the specific mass (# of protons and neutrons) for one atom of an element…usually an isotope

Question 18

11. What is the difference between atomic mass and mass number? When are mass numbers used?

Answer 18

Atomic mass is the average mass of all atoms of an element…found on PT
mass number is a specific mass for one specific atom of an element…used to show an isotope

Question 19

13. Compare and Contrast the following: Neutral atom, isotope, ion.

Answer 19

Neutral atoms have the same number of protons and electrons.
Isotopes have a different number of neutrons than protons.
Ions have more or less electrons than protons.

Question 20

14. What are valence electrons and why are they important?

Answer 20

They are in the outer shell of an atom. They are important because they determine what the element will bond to. (chemical properties)

Question 21

15. How many electrons are in

F -1

Answer 21

10

Question 22

How many electrons are in

Ca +2

Answer 22

18

Question 23

How many electrons are in

O-2

Answer 23

10

Question 24

How many electrons are in

K +1

Answer 24

18

Question 25

How many electrons are in | Li+1

Answer 25

2

Question 26

How many electrons are in | S-2

Answer 26

18

Question 27

How many electrons are in | N-3

Answer 27

10

Question 28

16. What is an isotope?

Answer 28

More neutrons than protons in nucleus.

Question 29

How do you write the name of an isotope?

Answer 29

Carbon-14, Uranium-238, Nitrogen-15, the number after element name tells you the mass number (specific mass for that atom)

Question 30

``` 17. What are the numbers of protons and neutrons in the following isotopes: carbon-13 uranium-235 Nitrogen-15 hydrogen-3 ```

Answer 30

Carbon-13 (6 protons, 7 neutrons) Uranium- 235 (92 Protons, 143 neutrons) Nitrogen-15 (7 protons, 8 neutrons) Hydrogen-3 (1 proton, 2 neutrons)

Question 31

18. What are the rows on the periodic table called? What do they tell you about the elements in that row?

Answer 31

Periods, they tell you how many shells an atom of that element has.

Question 32

19. What are the columns on the periodic table called? What do elements in the same column have in common?

Answer 32

Groups, they have the same number of valence electrons

Question 33

21. How can you determine the number of valence electrons for each element?

Answer 33

Oxidation #

Question 34

22. What group of elements are considered stable? How many e- do they have in their valence shell?

Answer 34

Noble gases, 8 valence electrons

Question 35

23. What 2 groups are the most reactive? Why is this?

Answer 35

Alkali metals and halogens, they are one valence electron away from becoming stable

Question 36

24. What are the 2 periodic trends?

Answer 36

Electronegativity (ionization energy) and atomic radius

Question 37

25. What is atomic radius?

Answer 37

The size of an atoms electron cloud

Question 38

26. What is electronegativity?

Answer 38

How strongly an atom attracts an electron

Question 39

28. How can you tell where the metals and non-metals are on the PT?

Answer 39

Metals are to the left of the staircase, non-metals are to the right

Question 40

29. Are most elements metals or non-metals?

Answer 40

metals

Question 41

30. What does an oxidation number tell you?

Answer 41

It tells you the charge of the ion formed by that element. It also tells you how many electrons are added or lost. +1 +2 +3 ±4 -3 -2 -1 0

Question 42

31. Compare ionic and covalent bonds. Include what electrons do and types of elements involved.

Answer 42

Ionic are between metals and non-metals and electrons are transferred. Covalent bonds are between non-metals and non-metals and electrons are shared.

Question 43

32. What is a cation and anion? What type of bond are they involved in?

Answer 43

Cation is a positive ion Anion is a negative ion Involved in ionic bonds…metal becomes cation, non-metal becomes anion

Question 44

33. Describe how metals and non-metals become ions in ionic bonds.

Answer 44

Metals lose electrons and become positive, non-metals gain electrons and become negative

Question 45

34. What are the rules for naming ionic compounds?

Answer 45

Metal goes first, add “ide” to end of the non-metal | Ex. Sodium Chloride

Question 46

35. What are the rules for naming ionic compounds that involve a transition metal?

Answer 46

If one element is a transition metal you write the name of the metal followed by a roman numeral that tells the charge of the metal atom. Then write the name of the anion with ide on the end, or the name of the polyatomic ion.

Question 47

What are the steps in the scientific method

Answer 47

``` Question Background research Hypothesis Experiment Results Conclusion Publish ```

Question 48

Label transition metals, metals, non metals, alkali earth metals, halogens, alkali metals, Nobel gases, hydrogen , and oxidation numbers

Answer 48

See chart

Question 49

36, what type of bond is this | P2S3

Answer 49

Covalent

Question 50

Name the compound MgCl2 Also, ionic or covalent

Answer 50

Magnesium chloride and it is ionic

Question 51

Name IrBr3 | Is the charge cation or anion

Answer 51

Iridium (Roman numeral three) bromide

Question 52

What type of bond would hydrogen and nitrogen form?

Answer 52

Covalent

Question 53

What type of bond would hydrogen and oxygen make

Answer 53

Covalent

Question 54

What is the difference between elements and compounds

Answer 54

Elements are all one type of atom | Compounds are two or more elements bonded together

Question 55

What is a molecule

Answer 55

Molecule is more than one atom bonded together | H2O, NaCl

Question 56

What is a mixture

Answer 56

Two elements or compounds that are not chemically bonded together N and O

Question 57

Give examples of physical changes

Answer 57

Water changing state, a piece of paper being crumpled, butter melting

Question 58

What are some indicators that a physical change has occurred

Answer 58

Object changed shape, no new compound or element created, reversible, no new properties( color)

Question 59

What are examples of chemical change

Answer 59

Anything burning or rusting

Question 60

What are some indicators that a chemical change has occurred

Answer 60

A new substance is created, color changes, odor, bubbles, new molecular structure, atoms rearranged, bonds broken